LabQuest 18 Chemistry with Vernier 18 - 1 Additi.docx
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LabQuest 18 Chemistry with Vernier 18 - 1 Additivity of Heats of Reaction: Hess’s Law In this experiment, you will use a Styrofoam-cup calorimeter to measure the heat released by three reactions. One of the reactions is the same as the combination of the other two reactions. Therefore, according to Hess’s law, the heat of reaction of the one reaction should be equal to the sum of the heats of reaction for the other two. This concept is sometimes referred to as the additivity of heats of reaction. The primary objective of this experiment is to confirm this law. The reactions we will use in this experiment are: (1) Solid sodium hydroxide dissolves in water to form an aqueous solution of ions. NaOH(s) Na+(aq) + OH–(aq) H1 = ? (2) Solid sodium hydroxide reacts with aqueous hydrochloric acid to form water and an aqueous solution of sodium chloride. NaOH(s) + H+(aq) ) + Cl–(aq) H2O(l) + Na+(aq) + Cl–(aq) H2 = ? (3) Solution s of aqueous sodium hydroxide and hydrochloric acid react to form water and aqueous sodium chloride. Na+(aq) + OH–(aq) + H+(aq) ) + Cl–(aq) H2O(l) + Na+(aq) + Cl–(aq) H3 = ? In the space below, combine two of the above equations algebraically to obtain the third equation. Indicate the number of each reaction on the shorter lines. ______ __________________________________________________________________ ______ __________________________________________________________________ ______ __________________________________________________________________ You will use a Styrofoam cup in a beaker as a calorimeter, as shown in Figure 1. For purposes of this experiment, you may assume that the heat loss to the calorimeter and the surrounding air is negligible. Even if heat is lost to either of these, it is a fairly constant factor in each part of the experiment, and has little effect on the final results. You will make three grand assumptions in this experiment: 1. The specific heat of solution is equivalent to the specific heat of water. 2. The density of solution is equivalent to the density of water. 3. All solutions are identical in temperature before mixing. OBJECTIVES In this experiment, you will Combine equations for two reactions to obtain the equation for a third reaction. Use a calorimeter to measure the temperature change in each of three reactions. Calculate the heat of reaction, H, for the three reactions. Use the results to confirm Hess’s law. LabQuest 18 18 - 2 Chemistry with Vernier MATERIALS LabQuest 4.00 g of solid NaOH LabQuest App ring stand Temperature Probe utility clamp 50 mL of 1.0 M NaOH stirring rod 50 mL of 1.0 M HCl Styrofoam cup 100 mL of 0.50 M HCl 250 mL beaker 100 mL of water PROCEDURE Reaction 1 1. Obtain and wear goggles. 2. Connect the Temperature Probe to LabQuest and choose New from the File menu. If you have an older sensor that does not auto-ID, manually ...
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Experiment 1 Calorimetry .docx
Experiment 1: Calorimetry
Post lab
Rawan Douar, Albert Campbell, Riley
Richardson, Christopher Cardenas
02/10/17
Instructor: Meng Chen
CHM2046L
Section: 912
Introduction
We determined the change in enthalpy to be negative, which means energy is sendoff the system and entering the environments in the form of heat.
Calorimetry is the chemical process which is used to measure heat in chemical reaction. The apparatus used is the calorimeter. A coffee cup calorimeter is not technologically advanced but it is effective in stopping heat transfer between the system and the atmosphere. Because the cup is open to the air, this is a constant pressure measurement. Per the first law of thermodynamics, the total energy of an isolated system can neither be created nor destroyed. In other words, energy is preserved in chemical reaction.
Calorimeter will consist of two nested Styrofoam coffee cups and a plastic cover. It will use a temperature sensor armed with a thermocouple probe. There will be a hole in the plastic cover of your calorimeter for insertion of the probe. In this experiment, we are going to study about the redox reactions with coffee cup and calorimeter.
Hypothesis and Objectives
Using a coffee cup calorimeter, the heat of neutralization of HCl and NaOH is measured. From this, the enthalpy change for the neutralization of one mole of HCl can be calculated.
· Introduction to the technique of calorimetry, in which the heat is evolved or absorbed by a chemical reaction is incidental by measuring temperature vicissitudes in an insulated reaction container.
· Reaction involve strong bases and acids will produce more heat.
Methods
Following are the materials that are used in experiment.
· Coffee cup calorimeter thermometer
· Lid or parafilm
· 10 mL graduated cylinder
· HCL
· NaOH
· Water
· 250 mL beaker
Procedure
1. Set up calorimeter apparatus.
2. Measuring solution temperature before mixing.
3. Adding simultaneously HCl and NaOH to the coffee cup.
4. Measure temperature change after mixing.
5. Calculate enthalpy change.
(J. Kotz, P. Treichel, J. Townsend; Chemistry & Chemical Reactivity 7th ed. 2009)
Obtain 10 ml of cold water and get the temperature, and pour it into your calorimeter. Then do the same thing for hot water. After that, measure the final temperature when it reaches equilibrium. Use the initial and the final temperatures to measure Ccal. Now gather two 50 mL beakers, one for NaOH, and one for HCl. Use the 10-mL graduated cylinder and then add the 3 mL of HCl and 7 mL of water, measure the temperature and put it into your unfilled calorimeter. Do the same for NaOH. Then put the thermometer in and measure the exact last temperature of it.
Clean up, and do the same thing aga ...
Catalyst Education 2020Enthalpy of Dissolution and Neutr
The document describes an experiment to determine the molar enthalpies of dissolution and neutralization reactions using calorimetry. Students will: (1) Determine the enthalpy of dissolving sodium hydroxide in water. (2) Determine the enthalpy of neutralizing sodium hydroxide and hydrochloric acid. (3) Use Hess's law to indirectly determine the enthalpy of dissolving sodium hydroxide from the first two reactions. Students will compare their results to literature values and each other.
Entalphy's Experiment report
The document reports on an experiment to determine the enthalpy change of the neutralization reaction between sodium hydroxide and hydrochloric acid. 150 mL of 1M HCl and 50 mL of 1M NaOH were mixed in a polystyrene cup calorimeter. The temperature increase of 0.75°C was used to calculate the energy transferred of 156.75 J. Thermochemistry principles are discussed including definition of enthalpy change, methods to determine it including calorimetry, and equations used to calculate energy from temperature change measurements in solution calorimetry.
Arizona State University 1 School of Molecular Sciences .docx
Arizona State University 1 School of Molecular Sciences
How Can the Thermodynamics of
Dissolution be Defined?
Introduction:
The Gibbs-Helmholtz equation expresses the relationship between the free-energy
change, the enthalpy change, and the entropy change at constant temperature and
pressure:
∆G = ∆H - T∆S Equation 1
From knowing the value of ∆G, you may predict whether a process/reaction will be
spontaneous at a certain temperature. A process is spontaneous if ∆G is negative (∆G <
0), nonspontaneous if ∆G is positive (∆G > 0), and at equilibrium if ∆G = 0.
The enthalpy change, ∆Hrxn, is the heat gained or lost by a system during a reaction
carried out at constant pressure. Most reactions occur in several steps, with energy
required (endothermic, positive ∆H) because energy is needed to break bonds, and
energy released (exothermic, negative ∆H) because energy is released as new bonds
are formed. ∆Hrxn represents the total change in heat energy or enthalpy over the course
of the reaction. In this experiment, you will use a coffee-cup calorimeter to determine the
heat absorbed or released during the dissolution of ammonium chloride and the
dissolution of calcium chloride. From observing the contents of the coffee-cup calorimeter,
you will decide whether the dissolution processes are spontaneous or nonspontaneous.
You will also calculate values of ∆Grxn to check your prediction.
From the law of conservation of energy (energy is conserved) the total energy for the
dissolution process is:
qsystem + qsurroundings = 0 or qsystem = - qsurroudnings Equation 2
where qsystem (or qrxn) represents the heat gained or lost by dissolving the solid (the
system), and qsurroundings (or qsolution) is the heat gained or lost by the solution in the
calorimeter (the surroundings). Thus, heat energy is essentially transferred between the
dissolving solid and the solution in the calorimeter. (For this experiment, the heat
absorbed by the cup, probe, and surroundings can be considered as negligible, so it is
not included in the expression above.)
The heat absorbed or released by the contents of the calorimeter is given by:
q = (mass solution)*(specific heat of solution)*(change in temperature)
q = m· Cs · T, where T=Tfinal-Tinitial Equation 3
The mass of the solution is the sum of the masses of the water and solid placed in the
calorimeter. (Recall that the density of water is1.00 g/mL.) Because the solution is very
Arizona State University 2 School of Molecular Sciences
dilute, the specific heat of the solution is basically equal to that of water, which is 4.184
J/gºC. To calculate change (∆) for a variable it is always final minus initial. The value of
qsurr can be calculated.
Lesson : Enthalpy and Calorimetry
This document provides an overview of exothermic and endothermic reactions, calorimetry, and how to calculate enthalpy changes. It discusses key concepts like:
1) The standard enthalpy change (ΔH°) is the enthalpy change measured under standard conditions of temperature and pressure.
2) Calorimetry can be used to determine enthalpy changes by measuring the temperature change of a reaction mixture in a calorimeter.
3) Sample problems demonstrate how to use calorimetry data like temperature changes, masses, and concentrations to calculate enthalpy changes for chemical reactions.
INTRODUCTIONChemical reactions are generally accompanied by some.docx
INTRODUCTION
Chemical reactions are generally accompanied by some heat change. The chemical reactions which involve energy changes are referred to as thermochemical reactions. During many chemical reactions, energy is converted to heat energy and result in increase in the temperature of the surrounding. These reactions are called exothermic reactions. Some chemical changes absorb energy from the surrounding and are known as endothermic reactions.
Enthalpy change always result from changes in a chemical system, hence, the heat changes are classified according to the type of chemical reactions. For instance, enthalpy change from the dissolution of a substance is called the heat of solution. The enthalpy change involved in a chemical change stays constant regardless of the route taken during the chemical change provided the initial and final conditions remain the same. This is the Hess' law of constant heat summation.
PROCEDURE
1. The heat of neutralization of HCl (aq) with NaOH (aq).
Using a graduated cylinder, about 50.0mL of 1.0M HCl was carefully measured and transferred into the calorimeter that was setup as instructed. Then 50.0mL ofNaOH into a small beaker. The stirring plate was then switched on and the stirring bar was adjusted until it spun rapidly and smoothly. The time duration was changed to 180 seconds in the LabQuest. The probe was checked to ensure it was placed properly in the calorimeter and the green arrow in the LabQuest was pressed to continue with the experiment. NaOH solution was added into the calorimeter after 40s. After data was taken, a graph was projected onto the display and the data was then analysed as instructed.
2. The heat of solution of NaOH (s)
About 4.00g of solid NaOH was carefully weighedusing a weighing bottle. Then 100mL of distilled water was carefully added into the calorimeter. The stirring plate was switched on and the stirring bar adjusted until it spun quickly and smoothly. The duration on the LabQuest was reset to 480s r. The probe was checked to ensure that it was beneath the liquid level. Solid NaOH was poured into the calorimeter after 40s. After data was obtained, it was then analysed using the procedure given.
3. The heat of reaction of HCl (aq) with NaOH (s)
About 55.0mL of 1.0M HCl was carefully measured using and poured into the calorimeter. Using the cylinder, 45.0mL of distilled water was carefully measured and poured into the calorimeter. About 2.00g of solid NaOH was carefully weighed in a capped vial. The stirring plate was switched on and the stirring bar adjusted until it spun quickly and smoothly. The duration on the LabQuest was reset to 480s . The temperature probe was properly placed in the calorimeter. Solid NaOH was added to the calorimeter after 40.5s. After the data was obtained, a drop of phenolphthalein indicator was added into the calorimeter and mixed well. The data was then analyzed following the instructions that were given.
DATA
1. The heat of neutralization of HCl (a.
Chemistry M4 Energetics
This document discusses energy changes that occur during chemical reactions. It defines endothermic and exothermic reactions, and explains how to interpret energy diagrams for these reactions. Key terms like activation energy, enthalpy change, heat of solution, and heat of neutralization are defined. The document provides examples of how to calculate heat of solution and heat of neutralization using experimental data and equations.
2016 topic 5.1 measuring energy changes
This document provides an overview of exothermic and endothermic reactions, calorimetry, and how to calculate enthalpy changes. The key points are:
- Exothermic reactions release heat while endothermic reactions absorb heat.
- Enthalpy change (ΔH) is the quantity of heat released or absorbed during a chemical reaction.
- Calorimetry experiments allow calculation of ΔH by measuring the temperature change of a reaction mixture.
- Sample problems demonstrate how to use calorimetry data like mass changes and temperature differences to calculate the enthalpy change for a reaction.
Recommended
Experiment 1 Calorimetry .docx
Experiment 1: Calorimetry
Post lab
Rawan Douar, Albert Campbell, Riley
Richardson, Christopher Cardenas
02/10/17
Instructor: Meng Chen
CHM2046L
Section: 912
Introduction
We determined the change in enthalpy to be negative, which means energy is sendoff the system and entering the environments in the form of heat.
Calorimetry is the chemical process which is used to measure heat in chemical reaction. The apparatus used is the calorimeter. A coffee cup calorimeter is not technologically advanced but it is effective in stopping heat transfer between the system and the atmosphere. Because the cup is open to the air, this is a constant pressure measurement. Per the first law of thermodynamics, the total energy of an isolated system can neither be created nor destroyed. In other words, energy is preserved in chemical reaction.
Calorimeter will consist of two nested Styrofoam coffee cups and a plastic cover. It will use a temperature sensor armed with a thermocouple probe. There will be a hole in the plastic cover of your calorimeter for insertion of the probe. In this experiment, we are going to study about the redox reactions with coffee cup and calorimeter.
Hypothesis and Objectives
Using a coffee cup calorimeter, the heat of neutralization of HCl and NaOH is measured. From this, the enthalpy change for the neutralization of one mole of HCl can be calculated.
· Introduction to the technique of calorimetry, in which the heat is evolved or absorbed by a chemical reaction is incidental by measuring temperature vicissitudes in an insulated reaction container.
· Reaction involve strong bases and acids will produce more heat.
Methods
Following are the materials that are used in experiment.
· Coffee cup calorimeter thermometer
· Lid or parafilm
· 10 mL graduated cylinder
· HCL
· NaOH
· Water
· 250 mL beaker
Procedure
1. Set up calorimeter apparatus.
2. Measuring solution temperature before mixing.
3. Adding simultaneously HCl and NaOH to the coffee cup.
4. Measure temperature change after mixing.
5. Calculate enthalpy change.
(J. Kotz, P. Treichel, J. Townsend; Chemistry & Chemical Reactivity 7th ed. 2009)
Obtain 10 ml of cold water and get the temperature, and pour it into your calorimeter. Then do the same thing for hot water. After that, measure the final temperature when it reaches equilibrium. Use the initial and the final temperatures to measure Ccal. Now gather two 50 mL beakers, one for NaOH, and one for HCl. Use the 10-mL graduated cylinder and then add the 3 mL of HCl and 7 mL of water, measure the temperature and put it into your unfilled calorimeter. Do the same for NaOH. Then put the thermometer in and measure the exact last temperature of it.
Clean up, and do the same thing aga ...
Catalyst Education 2020Enthalpy of Dissolution and Neutr
The document describes an experiment to determine the molar enthalpies of dissolution and neutralization reactions using calorimetry. Students will: (1) Determine the enthalpy of dissolving sodium hydroxide in water. (2) Determine the enthalpy of neutralizing sodium hydroxide and hydrochloric acid. (3) Use Hess's law to indirectly determine the enthalpy of dissolving sodium hydroxide from the first two reactions. Students will compare their results to literature values and each other.
Entalphy's Experiment report
The document reports on an experiment to determine the enthalpy change of the neutralization reaction between sodium hydroxide and hydrochloric acid. 150 mL of 1M HCl and 50 mL of 1M NaOH were mixed in a polystyrene cup calorimeter. The temperature increase of 0.75°C was used to calculate the energy transferred of 156.75 J. Thermochemistry principles are discussed including definition of enthalpy change, methods to determine it including calorimetry, and equations used to calculate energy from temperature change measurements in solution calorimetry.
Arizona State University 1 School of Molecular Sciences .docx
Arizona State University 1 School of Molecular Sciences
How Can the Thermodynamics of
Dissolution be Defined?
Introduction:
The Gibbs-Helmholtz equation expresses the relationship between the free-energy
change, the enthalpy change, and the entropy change at constant temperature and
pressure:
∆G = ∆H - T∆S Equation 1
From knowing the value of ∆G, you may predict whether a process/reaction will be
spontaneous at a certain temperature. A process is spontaneous if ∆G is negative (∆G <
0), nonspontaneous if ∆G is positive (∆G > 0), and at equilibrium if ∆G = 0.
The enthalpy change, ∆Hrxn, is the heat gained or lost by a system during a reaction
carried out at constant pressure. Most reactions occur in several steps, with energy
required (endothermic, positive ∆H) because energy is needed to break bonds, and
energy released (exothermic, negative ∆H) because energy is released as new bonds
are formed. ∆Hrxn represents the total change in heat energy or enthalpy over the course
of the reaction. In this experiment, you will use a coffee-cup calorimeter to determine the
heat absorbed or released during the dissolution of ammonium chloride and the
dissolution of calcium chloride. From observing the contents of the coffee-cup calorimeter,
you will decide whether the dissolution processes are spontaneous or nonspontaneous.
You will also calculate values of ∆Grxn to check your prediction.
From the law of conservation of energy (energy is conserved) the total energy for the
dissolution process is:
qsystem + qsurroundings = 0 or qsystem = - qsurroudnings Equation 2
where qsystem (or qrxn) represents the heat gained or lost by dissolving the solid (the
system), and qsurroundings (or qsolution) is the heat gained or lost by the solution in the
calorimeter (the surroundings). Thus, heat energy is essentially transferred between the
dissolving solid and the solution in the calorimeter. (For this experiment, the heat
absorbed by the cup, probe, and surroundings can be considered as negligible, so it is
not included in the expression above.)
The heat absorbed or released by the contents of the calorimeter is given by:
q = (mass solution)*(specific heat of solution)*(change in temperature)
q = m· Cs · T, where T=Tfinal-Tinitial Equation 3
The mass of the solution is the sum of the masses of the water and solid placed in the
calorimeter. (Recall that the density of water is1.00 g/mL.) Because the solution is very
Arizona State University 2 School of Molecular Sciences
dilute, the specific heat of the solution is basically equal to that of water, which is 4.184
J/gºC. To calculate change (∆) for a variable it is always final minus initial. The value of
qsurr can be calculated.
Lesson : Enthalpy and Calorimetry
This document provides an overview of exothermic and endothermic reactions, calorimetry, and how to calculate enthalpy changes. It discusses key concepts like:
1) The standard enthalpy change (ΔH°) is the enthalpy change measured under standard conditions of temperature and pressure.
2) Calorimetry can be used to determine enthalpy changes by measuring the temperature change of a reaction mixture in a calorimeter.
3) Sample problems demonstrate how to use calorimetry data like temperature changes, masses, and concentrations to calculate enthalpy changes for chemical reactions.
INTRODUCTIONChemical reactions are generally accompanied by some.docx
INTRODUCTION
Chemical reactions are generally accompanied by some heat change. The chemical reactions which involve energy changes are referred to as thermochemical reactions. During many chemical reactions, energy is converted to heat energy and result in increase in the temperature of the surrounding. These reactions are called exothermic reactions. Some chemical changes absorb energy from the surrounding and are known as endothermic reactions.
Enthalpy change always result from changes in a chemical system, hence, the heat changes are classified according to the type of chemical reactions. For instance, enthalpy change from the dissolution of a substance is called the heat of solution. The enthalpy change involved in a chemical change stays constant regardless of the route taken during the chemical change provided the initial and final conditions remain the same. This is the Hess' law of constant heat summation.
PROCEDURE
1. The heat of neutralization of HCl (aq) with NaOH (aq).
Using a graduated cylinder, about 50.0mL of 1.0M HCl was carefully measured and transferred into the calorimeter that was setup as instructed. Then 50.0mL ofNaOH into a small beaker. The stirring plate was then switched on and the stirring bar was adjusted until it spun rapidly and smoothly. The time duration was changed to 180 seconds in the LabQuest. The probe was checked to ensure it was placed properly in the calorimeter and the green arrow in the LabQuest was pressed to continue with the experiment. NaOH solution was added into the calorimeter after 40s. After data was taken, a graph was projected onto the display and the data was then analysed as instructed.
2. The heat of solution of NaOH (s)
About 4.00g of solid NaOH was carefully weighedusing a weighing bottle. Then 100mL of distilled water was carefully added into the calorimeter. The stirring plate was switched on and the stirring bar adjusted until it spun quickly and smoothly. The duration on the LabQuest was reset to 480s r. The probe was checked to ensure that it was beneath the liquid level. Solid NaOH was poured into the calorimeter after 40s. After data was obtained, it was then analysed using the procedure given.
3. The heat of reaction of HCl (aq) with NaOH (s)
About 55.0mL of 1.0M HCl was carefully measured using and poured into the calorimeter. Using the cylinder, 45.0mL of distilled water was carefully measured and poured into the calorimeter. About 2.00g of solid NaOH was carefully weighed in a capped vial. The stirring plate was switched on and the stirring bar adjusted until it spun quickly and smoothly. The duration on the LabQuest was reset to 480s . The temperature probe was properly placed in the calorimeter. Solid NaOH was added to the calorimeter after 40.5s. After the data was obtained, a drop of phenolphthalein indicator was added into the calorimeter and mixed well. The data was then analyzed following the instructions that were given.
DATA
1. The heat of neutralization of HCl (a.
Chemistry M4 Energetics
This document discusses energy changes that occur during chemical reactions. It defines endothermic and exothermic reactions, and explains how to interpret energy diagrams for these reactions. Key terms like activation energy, enthalpy change, heat of solution, and heat of neutralization are defined. The document provides examples of how to calculate heat of solution and heat of neutralization using experimental data and equations.
2016 topic 5.1 measuring energy changes
This document provides an overview of exothermic and endothermic reactions, calorimetry, and how to calculate enthalpy changes. The key points are:
- Exothermic reactions release heat while endothermic reactions absorb heat.
- Enthalpy change (ΔH) is the quantity of heat released or absorbed during a chemical reaction.
- Calorimetry experiments allow calculation of ΔH by measuring the temperature change of a reaction mixture.
- Sample problems demonstrate how to use calorimetry data like mass changes and temperature differences to calculate the enthalpy change for a reaction.
Thermochemistry ok1294993378
The document discusses energy changes that occur during chemical reactions. It defines exothermic and endothermic reactions, and standard enthalpy change. It provides examples of how to calculate enthalpy changes from experimental temperature change data using concepts like specific heat capacity. Hess's law, which states the enthalpy change of a reaction is equal to the sum of enthalpy changes of the steps in a reaction mechanism, is also introduced.
Chapter 4 Thermochemistry
This document discusses thermochemistry and energy changes that occur during chemical reactions. It defines exothermic and endothermic reactions, and how to construct energy level diagrams to represent them. Specific heats of reaction like combustion, precipitation, displacement, and neutralization are also explained. Experiments to determine various heats of reaction are described. The relationships between the heat of reaction and type of reactants, as well as the number of carbons in alcohols are also summarized.
BC Chemistry 162 Laboratory Manual Experiment 6 Vapor Press.docx
BC Chemistry 162 Laboratory Manual
Experiment 6: Vapor Pressure of Liquids
- 1 -
Experiment 6: Vapor Pressure of Liquids
Background
Liquids contain molecules that have different kinetic energies (due to different velocities). Some of the
faster liquid molecules have enough kinetic energy to vaporize. At the same time, some of the slower
vapor molecules condense into liquid. In an open container, the rate of vaporization will be greater than
the rate of condensation—hence, the liquid will eventually evaporate. In a sealed flask, however, there
will be a point in which equilibrium is reached between the rate of vaporization and the rate of
condensation. To the eye, it seems that the liquid doesn’t change at equilibrium. But at the microscopic
level a vapor molecule enters the liquid phase for every liquid molecule that enters the gas phase.
The total pressure in the sealed flask is due to the vaporized liquid plus air molecules present in the flask:
Ptotal = Pvapor + Pair (1)
In this experiment, you will investigate the relationship between
the vapor pressure of a liquid and its temperature. Pressure and
temperature data will be collected using a gas pressure sensor and
a temperature probe (Figure 1). Vapor pressures will be
determined by subtracting atmospheric pressure from the total
pressure.
The flask will be placed in water baths of different temperatures to
determine the effect of temperature on vapor pressure. You will
measure the vapor pressure of methanol and ethanol and
determine the enthalpy (heat) of vaporization for each liquid.
Objectives
In this experiment, you will
Investigate the relationship between the vapor pressure of a liquid and its temperature.
Compare the vapor pressure of two different liquids at the same temperature.
Use pressure‐temperature data and the Clausius‐Clapeyron equation to determine the heat of
vaporization for each liquid.
Caution!
The alcohols used in this experiment are flammable and poisonous. Avoid inhaling their vapors. Avoid
contacting them with your skin or clothing. Be sure there are no open flames in the lab during this
experiment. Notify your teacher immediately if an accident occurs.
Procedure
1. Wear goggles! You will work in pairs for this lab, but you may share water baths with your table.
2. Prepare four water baths: 20 to 25°C (use room temperature water), 30 to 35°C, 40 to 45°C, and 50 to
55°C. You should also have some hot water on a hot plate on reserve.
3. Obtain a temperature probe and gas pressure sensor. The sensor comes with a
rubber‐stopper assembly (Figure 2). The stopper has three holes, one of which
is closed. Make sure your tubing and valve are not inserted in the closed hole.
Insert the rubber‐stopper assembly into a 125 mL Erlenmeyer flask.
Important: Twist the stopper into the neck of the flask to ensure a tight
fit.
Figure 1
Figure 2
BC Ch.
Lecture of thermo-chemistry and calorimetery
This document discusses various concepts in thermochemistry including:
- Thermochemistry deals with thermal changes that accompany chemical and physical transformations. It aims to determine energy absorbed or released during reactions.
- Reactions require energy to overcome activation energy barriers to start, regardless of whether they are exothermic or endothermic. Exothermic reactions release excess energy to sustain the reaction while endothermic reactions require continuous energy input.
- Heat of formation is the energy absorbed or released when forming one mole of a substance from its elements. Hess's law allows calculating reaction energies using heats of formation without direct experimentation. Calorimetry is used to measure energy changes by determining temperature changes of a reaction mixture.
7-EnthalpyOfReaction
This document provides instructions on how to determine the enthalpy of a chemical reaction using calorimetry. Key points include:
1) Calorimetry involves measuring the temperature change of a reaction to calculate the heat released or absorbed.
2) Reactions can be exothermic (releasing heat) or endothermic (absorbing heat).
3) The enthalpy change (ΔH) of a reaction is an intensive property representing the heat of the reaction per mole.
4) Hess's law states that the enthalpy change of a reaction is independent of the pathway and can be determined from the sum of multiple steps.
D
This document describes an experiment using proton NMR spectroscopy to study the aquation kinetics of trans-dichlorotetraamminecobalt(III) chloride. The reaction involves one chloride ligand being replaced by a water molecule. Kinetic analysis of NMR peak heights and integrals over time indicates the reaction is first-order. Arrhenius and Eyring parameters are determined and used to calculate the rate constant at 25°C, which agrees with literature values. The positive entropy of activation suggests an associative mechanism for this substitution reaction.
Exp 11 Enthalpy
Here are the steps to solve this problem using Hess's Law:
1) Write the balanced equation for the reaction of interest:
NO(g) + O(g) → NO2(g)
2) Identify the relevant standard enthalpy change reactions:
2O3(g) → 3O2(g) ΔH° = -427 kJ
O2(g) → 2O(g) ΔH° = +495 kJ
NO(g) + O3(g) → NO2(g) + O2(g) ΔH° = -199 kJ
3) Rearrange the equations to obtain the overall reaction:
2O
Borax
This experiment aims to determine the thermodynamic parameters (ΔG°, ΔH°, ΔS°) for the dissolution of borax into borate ions in water at two temperatures. Students will prepare saturated borax solutions at room temperature and in an ice bath. They will titrate aliquots of the solutions with HCl to determine the borate ion concentration and calculate the solubility product (Ksp) at each temperature. Using the Ksp values and equations relating ΔG°, ΔH°, and ΔS° to temperature and Ksp, students can determine the thermodynamic parameters for this dissolution reaction. This will provide insight into whether the reaction is spontaneous and the roles of entropy and enthalpy.
To Determine the Enthalpy of H2O2 Decomposition in Aqueous Solution
This document summarizes an experiment to determine the enthalpy of decomposition of hydrogen peroxide in aqueous solution. The experiment involves first calibrating an isobaric calorimeter to determine its heat capacity. Then hydrogen peroxide solution is added to the calorimeter and manganese dioxide is used to catalyze the decomposition reaction. Temperature readings are taken before and after the reaction to determine the temperature change. The concentration of hydrogen peroxide is determined by titration and used to calculate moles reacted. From this, the enthalpy of decomposition is calculated to be -96 kJ/mole.
2 expt 1_phy_labmanual_pb
This document provides instructions for determining the heat capacity of a calorimeter. It involves mixing known quantities of hot and cold water in the calorimeter and measuring the temperature change. From the temperatures before and after mixing, and the masses and specific heat of water, the heat capacity of the calorimeter can be calculated using the formula provided. The experiment is carried out twice to obtain two values of heat capacity, which are then averaged to determine the final heat capacity.
Determination of the enthalpy of neutralisation
When a strong acid is neutralized with a strong base, a consistent amount of heat is released due to the formation of water from protons and hydroxyl ions. This experiment measures the temperature change during the neutralization of hydrochloric acid and potassium hydroxide to calculate the enthalpy of neutralization. A calorimeter is used to mix the reactants and measure the temperature change. Additionally, a known amount of electrical energy is input to determine the heat capacity of the system, allowing calculation of the enthalpy released during neutralization.
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The document discusses several experiments on factors that affect the rate of chemical reactions:
1. Particle size - Comparing the reaction of dilute HCl with large vs. small marble chips to see how particle size impacts the reaction rate. Smaller particles react faster due to a greater surface area.
2. Catalyst - Adding manganese dioxide speeds up the decomposition of hydrogen peroxide into oxygen and water, showing how a catalyst increases the reaction rate without being used up in the reaction.
3. Temperature - Measuring the time it takes for tablets to dissolve in hot, room temperature, and cold water, demonstrating that higher temperatures increase molecular motion and collision frequency, speeding up reactions.
Physical chemistry-experiment
1. The document provides instructions for an experiment to determine the heat of neutralization of hydrochloric acid (HCl) and sodium hydroxide (NaOH) through calorimetry.
2. Students are asked to measure the temperature change that occurs when 100mL of 0.2M HCl and 100mL of 0.2M NaOH are mixed in a calorimeter.
3. The temperature change is then used to calculate the heat of neutralization, which should be approximately -57.3 kJ/mol according to theory.
Test Document
This document provides instructions for an experiment to determine the heat of neutralization (ΔH) for acid-base reactions using calorimetry. It discusses key concepts like enthalpy, Hess' Law, and heat capacity. The procedure involves first calibrating thermometers and determining the heat capacity of the calorimeter. Then neutralization reactions between acids and bases are carried out in the calorimeter, and the temperature change is used to calculate the heat of reaction (ΔH) based on the calorimeter's heat capacity.
Notes for Unit 17 of AP Chemistry (Thermodynamics)
Notes for Unit 17 of AP Chemistry (Thermodynamics)
Determination of enthalpies of neutralization
This document outlines several experiments to determine enthalpy of neutralization reactions and apply Hess's law. It describes neutralizing strong acids with strong bases, weak acids with strong bases, and measuring the enthalpies of dissolving hydrochloric acid with ammonia and ammonium chloride in water. The experiments involve measuring temperature changes in a calorimeter when reactants are mixed and using the recorded temperature vs. time graphs to calculate the enthalpies of reaction.
Thermodynamics STUDENT NOTES.pptx
these notes indicate or talk about the concept of thermodynamics which deals with hot and cool temperatures
Heat
This document discusses heat and calorimetry in chemistry. It explains that calorimetry involves using a calorimeter to measure the heat absorbed or released during chemical or physical processes. A bomb calorimeter is used by food chemists to obtain calorie information on packaged foods by measuring the heat from combustion reactions. The document also discusses concepts such as heat of reaction, exothermic and endothermic reactions, enthalpy, and using the formula q = c × m × ΔT to calculate heat changes from calorimetry experiments.
E q u i l i b r i u m D e t e r m i n a t i o n o f a n E
E q u i l i b r i u m :
D e t e r m i n a t i o n o f a n E q u i l i b r i u m C o n s t a n t
P u r p o s e
To determine the equilibrium constant of a reaction.
L e a r n i n g O b j e c t i v e s
Take a reaction to equilibrium by setting up and monitoring a reaction in a reflux apparatus.
Measure the amount of acid at equilibrium by carrying out an acid-base titration.
Apply the information from a balanced chemical equation and data obtained in the laboratory to de-
termine the concentrations of reactants and products at equilibrium.
Calculate the value of the equilibrium constant using data obtained in the laboratory.
L a b o r a t o r y S k i l l s
To set up and monitor a reflux apparatus.
To carry out an acid-base titration.
E q u i p m e n t
Two 50-mL
graduated cylinders
Two 125-mL
Erlenmeyer flasks
1-mL pipet
25-mL buret
Equipment necessary
to assemble the
reflux apparatus
shown in Figure 1.
C h e m i c a l s
Anhydrous ethanol
(ethyl alcohol)
Anhydrous acetic
acid
Concentrated sulfuric
acid
I n t r o d u c t i o n
From the beginning of this course, we have generally assumed that chemical reactions go to completion, that is,
the reaction proceeds in the forward direction until one of the reactants is completely used up. However, many
reactions do not go to completion and are able to move both in the forward and reverse directions simultaneously.
Such a reaction is called a reversible reaction. A double arrow in the chemical equation designates a reversible
reaction, as shown in Reaction 1:
aA + bB −−−⇀↽−−− cC + dD (Reaction 1)
1
D e t e r m i n a t i o n o f a n E q u i l i b r i u m C o n s t a n t
A reversible reaction has two reaction rates: a forward reaction rate, where the reactants A and B are consumed
andtheproductsCandDareproduced,andareversereactionrate,wheretheproductsCandDareconsumedand
thereactantsAandBareproduced. Allreversiblereactionseventuallyreachapointatwhichtheforwardreaction
rate equals the reverse reaction rate. This point is called equilibrium. At equilibrium, the concentration of
reactants and products do not change with time. It is important to remember that even though the concentration
of reactants and products do not change with time, the reaction has not stopped. Equilibrium is a dynamic state.
The state will persist as long as the reaction conditions remain constant.
A reaction at equilibrium follows the law of mass action which gives the relationship between concentrations
of the reactants and products at equilibrium. According to the law of mass action, the relationship between
concentrations of reactants and products at equilibrium for the above reaction is given in Equation 1:
𝐾eq =
[C]𝑐[D]𝑑
[A]𝑎[B]𝑏
(Equation 1)
Thisrelationshipiscalledtheequilibrium-constantexpression. Theconstant, 𝐾eq, isapositivenumberwhose
value depends on the reaction and temperature.
In today’s experiment, students will be determining the equilibrium constant for the reac
Part 1.....InstructionsSelect one of the age groups disc.docx
Part 1.....
Instructions
Select one of the age groups discussed in this unit (adolescent, adult, or elderly). Create a community health strategy for dealing with intentional and unintentional injuries (motor vehicle accidents, suicide, or violence).Your response should include information on the morbidity and mortality rates and the key factors associated with the injuries.Your APA-Style essay must be at least two pages in length (not counting the title and reference pages). All sources used, including the textbook, must be referenced; paraphrased and quoted material must have accompanying citations.
Part 2....... Need To Be 1 Paragraph Long
According to the Centers for Medicare Services (CMS), the Affordable Care Act (ACA) was designed to give U.S. citizens improved flexibility and control, allowing them to make more informed decisions about their own health plans and healthcare providers.
Now that the ACA has been in place for several years, do you feel that in fact happened? Discuss the strengths and weaknesses of the ACA today.
.
Part 1 – Add to Website PlanList at least three .docx
Part 1 – Add to Website Plan
List
at least three interactive features that could be added to your
site and what purpose each would serve for your site and its visitors.
The form created in Part Two of this assignment can be included as
one of the interactive features.
Part 2 – Refine and finalize your website
Refine
and finalize your website by doing the following:
•
Add a simple web form—such as an order form, a subscription
to a newsletter, or a request for contact.
•
Use division or a table to structure the form elements.
•
Apply JavaScript
®
to validate the form.
•
Finalize a navigation system.
•
Use metadata to increase accessibility and search engine
optimization.
15
WEB/240 Version 1
8
•
Test for functionality and usability.
As in the prior assignment, use only Adobe
®
Dreamweaver
®
or
another HTML editor to refine the homepage developed in Week
Three.
Check
your HTML code using the Markup Validation Service on the
W3C
®
website, (www.w3.org) prior to submitting your web page(s).
A link to this site may be found in the Materials tab on your student
website.
Submit
all website files in a compressed folder.
.
More Related Content
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Thermochemistry ok1294993378
The document discusses energy changes that occur during chemical reactions. It defines exothermic and endothermic reactions, and standard enthalpy change. It provides examples of how to calculate enthalpy changes from experimental temperature change data using concepts like specific heat capacity. Hess's law, which states the enthalpy change of a reaction is equal to the sum of enthalpy changes of the steps in a reaction mechanism, is also introduced.
Chapter 4 Thermochemistry
This document discusses thermochemistry and energy changes that occur during chemical reactions. It defines exothermic and endothermic reactions, and how to construct energy level diagrams to represent them. Specific heats of reaction like combustion, precipitation, displacement, and neutralization are also explained. Experiments to determine various heats of reaction are described. The relationships between the heat of reaction and type of reactants, as well as the number of carbons in alcohols are also summarized.
BC Chemistry 162 Laboratory Manual Experiment 6 Vapor Press.docx
BC Chemistry 162 Laboratory Manual
Experiment 6: Vapor Pressure of Liquids
- 1 -
Experiment 6: Vapor Pressure of Liquids
Background
Liquids contain molecules that have different kinetic energies (due to different velocities). Some of the
faster liquid molecules have enough kinetic energy to vaporize. At the same time, some of the slower
vapor molecules condense into liquid. In an open container, the rate of vaporization will be greater than
the rate of condensation—hence, the liquid will eventually evaporate. In a sealed flask, however, there
will be a point in which equilibrium is reached between the rate of vaporization and the rate of
condensation. To the eye, it seems that the liquid doesn’t change at equilibrium. But at the microscopic
level a vapor molecule enters the liquid phase for every liquid molecule that enters the gas phase.
The total pressure in the sealed flask is due to the vaporized liquid plus air molecules present in the flask:
Ptotal = Pvapor + Pair (1)
In this experiment, you will investigate the relationship between
the vapor pressure of a liquid and its temperature. Pressure and
temperature data will be collected using a gas pressure sensor and
a temperature probe (Figure 1). Vapor pressures will be
determined by subtracting atmospheric pressure from the total
pressure.
The flask will be placed in water baths of different temperatures to
determine the effect of temperature on vapor pressure. You will
measure the vapor pressure of methanol and ethanol and
determine the enthalpy (heat) of vaporization for each liquid.
Objectives
In this experiment, you will
Investigate the relationship between the vapor pressure of a liquid and its temperature.
Compare the vapor pressure of two different liquids at the same temperature.
Use pressure‐temperature data and the Clausius‐Clapeyron equation to determine the heat of
vaporization for each liquid.
Caution!
The alcohols used in this experiment are flammable and poisonous. Avoid inhaling their vapors. Avoid
contacting them with your skin or clothing. Be sure there are no open flames in the lab during this
experiment. Notify your teacher immediately if an accident occurs.
Procedure
1. Wear goggles! You will work in pairs for this lab, but you may share water baths with your table.
2. Prepare four water baths: 20 to 25°C (use room temperature water), 30 to 35°C, 40 to 45°C, and 50 to
55°C. You should also have some hot water on a hot plate on reserve.
3. Obtain a temperature probe and gas pressure sensor. The sensor comes with a
rubber‐stopper assembly (Figure 2). The stopper has three holes, one of which
is closed. Make sure your tubing and valve are not inserted in the closed hole.
Insert the rubber‐stopper assembly into a 125 mL Erlenmeyer flask.
Important: Twist the stopper into the neck of the flask to ensure a tight
fit.
Figure 1
Figure 2
BC Ch.
Lecture of thermo-chemistry and calorimetery
This document discusses various concepts in thermochemistry including:
- Thermochemistry deals with thermal changes that accompany chemical and physical transformations. It aims to determine energy absorbed or released during reactions.
- Reactions require energy to overcome activation energy barriers to start, regardless of whether they are exothermic or endothermic. Exothermic reactions release excess energy to sustain the reaction while endothermic reactions require continuous energy input.
- Heat of formation is the energy absorbed or released when forming one mole of a substance from its elements. Hess's law allows calculating reaction energies using heats of formation without direct experimentation. Calorimetry is used to measure energy changes by determining temperature changes of a reaction mixture.
7-EnthalpyOfReaction
This document provides instructions on how to determine the enthalpy of a chemical reaction using calorimetry. Key points include:
1) Calorimetry involves measuring the temperature change of a reaction to calculate the heat released or absorbed.
2) Reactions can be exothermic (releasing heat) or endothermic (absorbing heat).
3) The enthalpy change (ΔH) of a reaction is an intensive property representing the heat of the reaction per mole.
4) Hess's law states that the enthalpy change of a reaction is independent of the pathway and can be determined from the sum of multiple steps.
D
This document describes an experiment using proton NMR spectroscopy to study the aquation kinetics of trans-dichlorotetraamminecobalt(III) chloride. The reaction involves one chloride ligand being replaced by a water molecule. Kinetic analysis of NMR peak heights and integrals over time indicates the reaction is first-order. Arrhenius and Eyring parameters are determined and used to calculate the rate constant at 25°C, which agrees with literature values. The positive entropy of activation suggests an associative mechanism for this substitution reaction.
Exp 11 Enthalpy
Here are the steps to solve this problem using Hess's Law:
1) Write the balanced equation for the reaction of interest:
NO(g) + O(g) → NO2(g)
2) Identify the relevant standard enthalpy change reactions:
2O3(g) → 3O2(g) ΔH° = -427 kJ
O2(g) → 2O(g) ΔH° = +495 kJ
NO(g) + O3(g) → NO2(g) + O2(g) ΔH° = -199 kJ
3) Rearrange the equations to obtain the overall reaction:
2O
Borax
This experiment aims to determine the thermodynamic parameters (ΔG°, ΔH°, ΔS°) for the dissolution of borax into borate ions in water at two temperatures. Students will prepare saturated borax solutions at room temperature and in an ice bath. They will titrate aliquots of the solutions with HCl to determine the borate ion concentration and calculate the solubility product (Ksp) at each temperature. Using the Ksp values and equations relating ΔG°, ΔH°, and ΔS° to temperature and Ksp, students can determine the thermodynamic parameters for this dissolution reaction. This will provide insight into whether the reaction is spontaneous and the roles of entropy and enthalpy.
To Determine the Enthalpy of H2O2 Decomposition in Aqueous Solution
This document summarizes an experiment to determine the enthalpy of decomposition of hydrogen peroxide in aqueous solution. The experiment involves first calibrating an isobaric calorimeter to determine its heat capacity. Then hydrogen peroxide solution is added to the calorimeter and manganese dioxide is used to catalyze the decomposition reaction. Temperature readings are taken before and after the reaction to determine the temperature change. The concentration of hydrogen peroxide is determined by titration and used to calculate moles reacted. From this, the enthalpy of decomposition is calculated to be -96 kJ/mole.
2 expt 1_phy_labmanual_pb
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Determination of the enthalpy of neutralisation
When a strong acid is neutralized with a strong base, a consistent amount of heat is released due to the formation of water from protons and hydroxyl ions. This experiment measures the temperature change during the neutralization of hydrochloric acid and potassium hydroxide to calculate the enthalpy of neutralization. A calorimeter is used to mix the reactants and measure the temperature change. Additionally, a known amount of electrical energy is input to determine the heat capacity of the system, allowing calculation of the enthalpy released during neutralization.
TOPIC 5. RATE OF REACTION-LAB
The document discusses several experiments on factors that affect the rate of chemical reactions:
1. Particle size - Comparing the reaction of dilute HCl with large vs. small marble chips to see how particle size impacts the reaction rate. Smaller particles react faster due to a greater surface area.
2. Catalyst - Adding manganese dioxide speeds up the decomposition of hydrogen peroxide into oxygen and water, showing how a catalyst increases the reaction rate without being used up in the reaction.
3. Temperature - Measuring the time it takes for tablets to dissolve in hot, room temperature, and cold water, demonstrating that higher temperatures increase molecular motion and collision frequency, speeding up reactions.
Physical chemistry-experiment
1. The document provides instructions for an experiment to determine the heat of neutralization of hydrochloric acid (HCl) and sodium hydroxide (NaOH) through calorimetry.
2. Students are asked to measure the temperature change that occurs when 100mL of 0.2M HCl and 100mL of 0.2M NaOH are mixed in a calorimeter.
3. The temperature change is then used to calculate the heat of neutralization, which should be approximately -57.3 kJ/mol according to theory.
Test Document
This document provides instructions for an experiment to determine the heat of neutralization (ΔH) for acid-base reactions using calorimetry. It discusses key concepts like enthalpy, Hess' Law, and heat capacity. The procedure involves first calibrating thermometers and determining the heat capacity of the calorimeter. Then neutralization reactions between acids and bases are carried out in the calorimeter, and the temperature change is used to calculate the heat of reaction (ΔH) based on the calorimeter's heat capacity.
Notes for Unit 17 of AP Chemistry (Thermodynamics)
Notes for Unit 17 of AP Chemistry (Thermodynamics)
Determination of enthalpies of neutralization
This document outlines several experiments to determine enthalpy of neutralization reactions and apply Hess's law. It describes neutralizing strong acids with strong bases, weak acids with strong bases, and measuring the enthalpies of dissolving hydrochloric acid with ammonia and ammonium chloride in water. The experiments involve measuring temperature changes in a calorimeter when reactants are mixed and using the recorded temperature vs. time graphs to calculate the enthalpies of reaction.
Thermodynamics STUDENT NOTES.pptx
these notes indicate or talk about the concept of thermodynamics which deals with hot and cool temperatures
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This document discusses heat and calorimetry in chemistry. It explains that calorimetry involves using a calorimeter to measure the heat absorbed or released during chemical or physical processes. A bomb calorimeter is used by food chemists to obtain calorie information on packaged foods by measuring the heat from combustion reactions. The document also discusses concepts such as heat of reaction, exothermic and endothermic reactions, enthalpy, and using the formula q = c × m × ΔT to calculate heat changes from calorimetry experiments.
E q u i l i b r i u m D e t e r m i n a t i o n o f a n E
E q u i l i b r i u m :
D e t e r m i n a t i o n o f a n E q u i l i b r i u m C o n s t a n t
P u r p o s e
To determine the equilibrium constant of a reaction.
L e a r n i n g O b j e c t i v e s
Take a reaction to equilibrium by setting up and monitoring a reaction in a reflux apparatus.
Measure the amount of acid at equilibrium by carrying out an acid-base titration.
Apply the information from a balanced chemical equation and data obtained in the laboratory to de-
termine the concentrations of reactants and products at equilibrium.
Calculate the value of the equilibrium constant using data obtained in the laboratory.
L a b o r a t o r y S k i l l s
To set up and monitor a reflux apparatus.
To carry out an acid-base titration.
E q u i p m e n t
Two 50-mL
graduated cylinders
Two 125-mL
Erlenmeyer flasks
1-mL pipet
25-mL buret
Equipment necessary
to assemble the
reflux apparatus
shown in Figure 1.
C h e m i c a l s
Anhydrous ethanol
(ethyl alcohol)
Anhydrous acetic
acid
Concentrated sulfuric
acid
I n t r o d u c t i o n
From the beginning of this course, we have generally assumed that chemical reactions go to completion, that is,
the reaction proceeds in the forward direction until one of the reactants is completely used up. However, many
reactions do not go to completion and are able to move both in the forward and reverse directions simultaneously.
Such a reaction is called a reversible reaction. A double arrow in the chemical equation designates a reversible
reaction, as shown in Reaction 1:
aA + bB −−−⇀↽−−− cC + dD (Reaction 1)
1
D e t e r m i n a t i o n o f a n E q u i l i b r i u m C o n s t a n t
A reversible reaction has two reaction rates: a forward reaction rate, where the reactants A and B are consumed
andtheproductsCandDareproduced,andareversereactionrate,wheretheproductsCandDareconsumedand
thereactantsAandBareproduced. Allreversiblereactionseventuallyreachapointatwhichtheforwardreaction
rate equals the reverse reaction rate. This point is called equilibrium. At equilibrium, the concentration of
reactants and products do not change with time. It is important to remember that even though the concentration
of reactants and products do not change with time, the reaction has not stopped. Equilibrium is a dynamic state.
The state will persist as long as the reaction conditions remain constant.
A reaction at equilibrium follows the law of mass action which gives the relationship between concentrations
of the reactants and products at equilibrium. According to the law of mass action, the relationship between
concentrations of reactants and products at equilibrium for the above reaction is given in Equation 1:
𝐾eq =
[C]𝑐[D]𝑑
[A]𝑎[B]𝑏
(Equation 1)
Thisrelationshipiscalledtheequilibrium-constantexpression. Theconstant, 𝐾eq, isapositivenumberwhose
value depends on the reaction and temperature.
In today’s experiment, students will be determining the equilibrium constant for the reac
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Notes for Unit 17 of AP Chemistry (Thermodynamics)
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E q u i l i b r i u m D e t e r m i n a t i o n o f a n E
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Part 1.....
Instructions
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Part 1 – Add to Website PlanList at least three .docx
Part 1 – Add to Website Plan
List
at least three interactive features that could be added to your
site and what purpose each would serve for your site and its visitors.
The form created in Part Two of this assignment can be included as
one of the interactive features.
Part 2 – Refine and finalize your website
Refine
and finalize your website by doing the following:
•
Add a simple web form—such as an order form, a subscription
to a newsletter, or a request for contact.
•
Use division or a table to structure the form elements.
•
Apply JavaScript
®
to validate the form.
•
Finalize a navigation system.
•
Use metadata to increase accessibility and search engine
optimization.
15
WEB/240 Version 1
8
•
Test for functionality and usability.
As in the prior assignment, use only Adobe
®
Dreamweaver
®
or
another HTML editor to refine the homepage developed in Week
Three.
Check
your HTML code using the Markup Validation Service on the
W3C
®
website, (www.w3.org) prior to submitting your web page(s).
A link to this site may be found in the Materials tab on your student
website.
Submit
all website files in a compressed folder.
.
Part 1 True or False Questions. (10 questions at 1 point each).docx
Part 1: True or False Questions.
(10 questions at 1 point each)
T
F
A hash algorithm uses a one-way cryptographic function, whereas both secret-key and public-key systems use two-way (i.e., reversible) cryptographic functions.
Answer: _____
T
F
The strongest 3DES (Triple DES) requires the use of three independent keys.
Answer: _____
T
F
When it comes to the ethics of a particular situation, there is only one right answer.
Answer: _____
T
F
Packet filters protect networks by blocking packets based on the packets’ contents.
Answer: _____
T
F
The biggest advantage of
public-key
cryptography over
secret-key
cryptography is in the area of key management/key distribution.
Answer: _____
T
F
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Answer: _____
T
F
Intrusion Detection Systems (IDS) provide no protection from internal threats.
Answer: _____
T
F
A Denial-of-Service attack does not require the attacker to penetrate the target's security defenses.
Answer: _____
T
F
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Answer: _____
T
F
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Answer: _____
Part 2: Multiple Choice Questions. Print
all
the correct answers in the blank following the question; in some cases a fully correct answer may require more than one lettered choice to be selected. (
Each question is worth 2 points.
There is no guarantee of partial credit for partially correct answers.)
If person A uses AES to transmit an encrypted message to person B, which key or keys will A have to use:
a.
A’s private key
b.
A’s public key
c.
B’s private key
d.
B’s public key
e.
None of the keys listed above
Answer(s): ____
From the perspective of
entropy
:
Plaintext will have a higher entropy than the ciphertext
The unequal frequency of characters in human languages tends to reduce the entropy of plaintext messages in that language
Encrypted messages appear to be noise-like
Plaintext requires more transmission bandwidth than ciphertext
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a.
A patent
b.
A copyright
c.
A patent and copyright
d.
Ethical standards
e.
All of the above
Answer(s): _____
Security
threats
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a.
Unlocked doors
b.
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c.
Hurricanes
d.
Un-patched software programs
e.
All of the above
Answer(s): _____
Denial of service attacks include:
a.
DNS poisoning
b.
Smurf attack
c.
Ping of death
d.
SYN flood
e.
All of the above
Answer(s): _____
Part 3: Short Answer Questions.
(10 questions at 5 points each)
Alan and Beatrice are both users of PKI. Explain how they use their keys to communicate when Alan sends a private message to Beatrice, and provides proof that he sent the message.
Answer:
Briefly describe the purpose of firewalls and how .
Part 11. Why is it so important in system engineering to become .docx
Part 1
1. Why is it so important in system engineering to become familiar with some of the analytical methods?
2. Identify and describe some of the technologies that are being applied in the design process. Provide some examples of typical applications, and describe some of the benefits associated with the application of computerized methods in the design process.
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Part 3
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Part 1: Using the internet, search for commercial IDPS systems. What classification systems and descriptions are used and how can these be used to compare the features and components of each IDPS? Create a comparison spreadsheet identifying the classification systems you find.
Part 2: What are some of the legal and ethical issues surrounding the use of intrusion detection systems logs and other technology tools as evidence in criminal and legal matters?
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Part 4:
Why is it so important in system engineering to become familiar with some of the analytical methods?
Identify and describe some of the technologies that are being applied in the design process. Provide some examples of typical applications, and describe some of the benefits associated with the application of computerized methods in the design process.
How does CAM and CAS relate to system engineering? Describe some possible impacts.
How is design review and evaluation accomplished? Why is it important relative to meeting system engineering objectives? Describe some of the checks and balances in the design process.
What is included in the establishment of a "functional” baseline, Allocated baseline, and Product baseline? Why is baseline management important?
What is configuration management (CM) and how does it relate to system engineering? Define Configuration Identification (CI) and Configuration Status Accounting (CSA).
Part 5: Select a system of your choice, and construct a sequential flow diagram of the overall system development process. Identify the major tasks in system development, and develop a plan/schedule of formal design review. Briefly describe what is covered in each.
Part 6:
Discuss some of the problems associated with the application of computerized methods in the design process. Provide examples. What cautions must be observed?
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Part 1- Create an outline of the assignment below then
Part 2-1000 word assignment
Your fast-food franchise has been cleared for business in all 4 countries (United Arab Emirates, Israel, Mexico, and China). You now have to start construction on your restaurants. The financing is coming from the United Arab Emirates, the materials are coming from Mexico and China, the engineering and technology are coming from Israel , and the labor will be hired locally within these countries by your management team from the United States. You invite all of the players to the headquarters in the United States for a big meeting to explain the project and get to know one another. The people seem to be staying with their own groups and not mingling.
What is the cultural phenomenon at play here (what is it called/ term)?
How do you explain the lack of intercultural communication and interaction?
What do you know about these cultures—specifically their economic, political, educational, and social systems—that could help you in getting them together?
What are some of the contrasting cultural values of these countries?
You are concerned about some of the language barriers as you start the meeting, particularly the fact that the United States is a low-context country, and some of the countries present are high-context countries. Furthermore, you only speak English, and you do not have an interpreter present.
How will this affect the presentation?
What are some of the issues you should be concerned about regarding verbal and nonverbal language for this group?
What strategy would you use to begin to have everyone develop a relationship with each other that will help ease future negotiations, development, and implementation?
.
Part 1 Review QuestionsWhat is the difference between criminal la.docx
Part 1: Review Questions
What is the difference between criminal law and civil law?
What is privacy, in the context of information security?
What is intellectual property? Is it offered the same protection in every country of the world? What laws currently protect it in the U.S. and Europe?
What are the three general categories of unethical and illegal behavior?
Part 2: Module Practice
What does CISSP stand for? Using the Internet, find out what continuing education is required in order for the holder of a CISSP to remain current and in good standing.
.
Part 1 Review QuestionsWhat is the difference between authenticat.docx
The document contains two parts. Part 1 lists review questions about authentication vs authorization, network security relationships, network vs host intrusion detection systems, and VPNs. Part 2 instructs the reader to create a spreadsheet that encrypts values using a transposition cipher, then further encrypts the results using a substitution cipher.
Part 1 SQLDatabase workScenarioDevelopment of a relationa.docx
Part 1: SQL/Database work
Scenario
Development of a relational database system for a food producing company
FoodRU is a Leicester-based food producing company. The company wants to keep details regarding both past and present employees and their assignment to shifts over time. At present, there are three defined shift patterns; the morning shift starts at 6am and finishes at 2pm, the day shift starts at 9am and finishes at 5pm, and the evening shift starts at 4pm and finishes at 12am (midnight). However, management have already indicated that they may need to add further shift patterns in the future (e.g., by adding a night shift to the existing ones so that the company can meet a high user demand for their foods). They therefore require shift details to be stored within a separate Shift table, with attributes that allow the storage of a shift name with its associated start and finish times (use the 24 hour clock for these times).
Past and present employee details are to be kept in the same Employee table, and the details to be kept are the employee’s unique 6 digit reference number, the first name, surname and any other names (if there are any) of the employee, the employee’s gender, contact address and contact telephone, the date on which the employee started his/her employment at the company and the date on which the employee finished his/her employment at the company (should s/he be a past employee). Details regarding staff assignments to shifts include the date that an employee was allocated to work a particular shift, and the date that s/he was taken off the shift (if not still assigned to it). Employees can be assigned to different shifts over time and even to the same shift over different time periods, although they cannot be assigned to more than one shift at any one time. A new employee may not yet be assigned to a shift.
Tasks:
1. Provide the table specifications for the THREE tables that are required by FoodRU to store employee, shift and assignment details. That is, for each of the three tables, you should provide, in a suitable presentation format, the name of the table and a specification of each its attributes to include:
• Attribute name
• Attribute brief description as to its meaning
• a description of the attribute’s data type/integrity (e.g., date field, character field of length 20, number field <= 10, etc. – you can use the Oracle data types within these descriptions if you want to)
• An indication as to whether the attribute is a primary key attribute and/or foreign key attribute
• An indication as to whether the attribute can or cannot take null values
Make sure your design specifies the appropriate links between the three tables. Remember to write down any additional integrity you need to enforce either at a specific table level or across two or more tables, if this is required. Also, remember to write down any justifications for the data types/integrity or for any other design features that.
Part 1 Review QuestionsWhat functions constitute a complete infor.docx
Part 1: Review Questions
What functions constitute a complete information security program?
What is the typical size of the security staff in a small organization? A medium-sized organization? A large organization? A very large organization?
Where can an organization place the information security unit? Where should (and shouldn’t) it be placed?
Into what four areas should the information security functions be divided?
Part 2: Module Practice
Design three security posters on various aspects of information security using a graphics presentation program and clip art. Describe the methods you used to develop your design.
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Part 1A persons lifestyle has a significant influence on the p.docx
Part 1:
A person's lifestyle has a significant influence on the person's health and development as he or she moves into middle age (and old age). Stability and change are also common factors in an adult's life.
Describe how middle adulthood provides stability in a person's life. Explain some of the factors that would lead to stability in a person's life as he or she moves through middle age.
Describe some of the more common lifestyle issues that have a negative impact on a person's continued development. Explain how a person may be able to reverse some of the lifestyle influences.
On the basis of your readings, describe what is meant by a midlife crisis. Explain why a midlife crisis may or may not be critical.
Part 2:
Erikson, Gould, Helson, and Levinson provide different perspectives on middle age in adulthood.
Describe each of these theories as it relates to middle adulthood.
On the basis of your readings, compare and contrast these theories. Which one gives a better explanation of middle adulthood?
Justify your answers with appropriate reasoning and research from your text and course readings. Comment on the postings of at least two peers, and provide an analysis of each peer’s postings while also suggesting specific additions or clarifications for improving the discussion question response.
.
Part 1 Review QuestionsWhat is the definition of information secu.docx
Part 1: Review Questions
What is the definition of information security? What essential protections must be in place to protect information systems from danger?
Define the InfoSec processes of identification, authentication, authorization, and accountability.
Define project management. Why is project management of particular interest in the field of information security?
What are the five basic outcomes that should be achieved through information security governance?
What is a threat in the context of information security? How many categories of threats exist as presented in this chapter?
Part 2: Module Practice
Find an article that talks about relative risk either from inside the organization or form external sources. Once you locate and read it, compose a 1-2 page paper that summarizes your findings and critique the article. Use a word processor to complete your assignment and submit it as a .docx or .doc document.
.
Part 1 Review QuestionsWhat is a security modelWhat are the es.docx
Part 1: Review Questions
What is a security model?
What are the essential processes of access control?
Identify at least two different approaches used to categorize access control methodologies. List the types of controls found in each.
What is COBIT? Who is its sponsor? What does it accomplish?
What is the standard of due care? How does it relate to due diligence?
What is baselining? How does it differ from benchmarking?
Part 2: Module Practice
Make a list of at least ten information security metrics that could be collected for a small internet commerce company with 10 employees. For this senario, the company uses an outside vendor for packaging and distribution. Whom should the metrics be reported?
.
Part 1 Listed below are several key Supreme Court decisions that .docx
Part 1:
Listed below are several key Supreme Court decisions that resulted in a clarification of inmate rights.
Choose any one
of the cases listed below. Summarize the facts of the case, the issue that needed to be resolved, the court’s decision, and the reasoning behind the decision.
Helling v. McKinney
(1993)
Washington v. Harper
(1990)
Hudson v. Palmer
(1984)
Bell v. Wolfish
(1979)
Bounds v. Smith
(1977)
Estelle v. Gamble
(1976)
Wolff v. McDonnell
(1974)
.
Part 1 Infrastructure DesignCreate an 8–10-page infrastructur.docx
Part 1: Infrastructure Design
Create an 8–10-page infrastructure design document in which you:
Identify the major hardware and software components of your hypothetical e-commerce company's information systems infrastructure.
Design your e-commerce company's hardware (database and proxy servers, network equipment) and software (analytics, big data, API, content management) from a size, scale, type, and interoperability standards perspective.
Document the potential security vulnerabilities and a security design for your e-commerce company.
Use graphical tools to create a data flow diagram (DFD) for your e-commerce company.
Use sources to support your writing.
Choose sources that are credible, relevant, and appropriate.
Cite each source listed on your source page at least one time within your assignment.
Part 2: Updated Gantt Chart
Use Microsoft Project to update the previously created Gantt chart with the major and minor tasks identified in the infrastructure design document.
.
part 1 I attended an international conference on Biotechnology and .docx
part 1: I attended an international conference on Biotechnology and one of the sessions I went to was on the subject of bio-engineering a "death gene" that could be introduced into the mosquito population and destroy every mosquito on earth. The discussion that ensued was about the ethics of such a thing. I want you to tell how you feel about introducing such a gene. Look up something about this. Your reference does not have to be about this particular gene, but can be about anything that relates to the discussion. Remember to cite your reference, and write at least 150 words
part 2:
Respond to another student
respond to this
I think that with regulation of the mosquito communities would be a good thing. Mosquitos carry many dangerous diseases and if we can lower the population we can slow the rate of transmission of these diseases. This could save many many lives around the world. I would be hesitant though to release the genetically engineered mosquitos into the environment. In the article I read they releases sterile male mosquitos into the environment. This I feel is a safer way to regulate because we are not altering any genes we are just regulating a naturally occurring issue in nature. Sterile males cannot pass on the genes and also male mosquitos are not the ones who would be likely to pass on the diseases. The article stated that only females bite and therefore males would not be capable of spreading the diseases. With sterile males being released there will be less mosquitos due to lack of repopulation. This will still allow organisms relying on mosquitos for food to still be able to survive with less risk to humans. They are an invasive species so it would help to eliminate the spread of mosquitos to different areas. This will keep the spread of disease throughout areas. I do not think it is right to alter the genes for human use though. It is not how nature had intended. If the gene pops up naturally in the population then it should not be taken out but we should not introduce it due to humans "playing God" with genetics. "Mosquitoes Engineered To Kill Their Own Kind." NPR. NPR, n.d. Web. 22 July 2014. .
.
Part 1 Chapter 7 Summary plus end of chapter discussion of Alfred.docx
Part 1:
Chapter 7 Summary plus end of chapter discussion of Alfred Marshall, should be 100-250 words
Part 2: The discussion on the first 7 pages is a satire on the economists (known as the neoclassical economists).
List 4 passages that can be considered satire.
(You need not write the entire passage.
Simply show clearly where the passage begins and ends.)
.
Parent Involvement Plan This week you will create a Parent Involve.docx
Parent Involvement Plan
This week you will create a Parent Involvement Plan in response to the following scenario:
Imagine you are working with infant, toddler and preschool aged children in a child care center. The majority of the children has special needs and receives early intervention or are on an IEP. Many of the children’s parents work two jobs and have a difficult time participating in the center's activities. Whenever the center plans an event, the parental involvement is lower than desired. The center has tried to increase parental involvement through such methods as calling to remind parents and sending home notices, but is not having any luck.
Your assignment is to create a Parental Involvement Plan to encourage better participation from parents. Follow these steps to develop your plan:
Step 1:
Identify the issue, discuss your beliefs about the situation, and formulate conclusions and offer suggestions to the director of the child care center.
Step 2:
Create a Parent Involvement Plan that your director can copy and paste into the employee and parent handbook. Your plan should include:
The importance of early intervention and individual educational plans
Ways to assist students and their families
The importance of parent involvement
Please use the template provided and your rubric as your guide to completing this assignment.
.
Parenting Practices Over GenerationsGeneration 1 Years children.docx
Parenting Practices Over Generations
Generation 1: Years children were raised (19XX-XXXX)
Generation 2: Years
Generation 3: Years
Parenting Practice 1: Education
Parenting Practice 2:
Parenting Practice 3:
Parenting Practice 4:
.
ParamsThe interface must be pleasing to look at (a basic form wit.docx
Params:
The interface must be pleasing to look at (a basic form with the four fields listed below, a playlist queue (checked listbox) and media player will suffice).
There must be a separate file that will contain information about each soundtrack in your system. That information will be:
Title;
Artist;
Note area;
Type; and
Anything else that you wish to include on each record.
There must be a way to add data to this file.
There must be a way to delete data from this file.
There must be at least one report using data from the file.
There must be a queue to allow you to play selected music tracks in sequence (like two in a row) without manual intervention.
There must be a way to show the data in at least two different sequences (by title, by artist, etc.).
There must be documentation explaining how your Jukebox works (how you add songs, play songs, etc.).
Currently there is a Text file that contains the information about the wav files to be played, several wav files that the text file references. I have also made an access database from the text file.
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LabQuest 18 Chemistry with Vernier 18 - 1 Additi.docx
- 1. LabQuest 18 Chemistry with Vernier 18 - 1 Additivity of Heats of Reaction: Hess’s Law In this experiment, you will use a Styrofoam-cup calorimeter to measure the heat released by three reactions. One of the reactions is the same as the combination of the other two reactions. Therefore, according to Hess’s law, the heat of reaction of the one reaction should be equal to the sum of the heats of reaction for the other two. This concept is sometimes referred to as the additivity of heats of reaction. The primary objective of this experiment is to confirm this law. The reactions we will use in this experiment are: (1) Solid sodium hydroxide dissolves in water to form an aqueous solution of ions. NaOH(s) Na+(aq) + OH–(aq) H1 = ? (2) Solid sodium hydroxide reacts with aqueous hydrochloric acid to form water and an aqueous solution of sodium chloride. NaOH(s) + H+(aq) ) + Cl–(aq) H2O(l) + Na+(aq) + Cl–(aq) H2 = ? (3)
- 2. Solution s of aqueous sodium hydroxide and hydrochloric acid react to form water and aqueous sodium chloride. Na+(aq) + OH–(aq) + H+(aq) ) + Cl–(aq) H2O(l) + Na+(aq) + Cl–(aq) H3 = ? In the space below, combine two of the above equations algebraically to obtain the third equation. Indicate the number of each reaction on the shorter lines. ______ _____________________________________________________ _____________ ______ _____________________________________________________ _____________ ______ _____________________________________________________ _____________
- 3. You will use a Styrofoam cup in a beaker as a calorimeter, as shown in Figure 1. For purposes of this experiment, you may assume that the heat loss to the calorimeter and the surrounding air is negligible. Even if heat is lost to either of these, it is a fairly constant factor in each part of the experiment, and has little effect on the final results. You will make three grand assumptions in this experiment: 1. The specific heat of solution is equivalent to the specific heat of water. 2. The density of solution is equivalent to the density of water. 3. All solutions are identical in temperature before mixing. OBJECTIVES In this experiment, you will Combine equations for two reactions to obtain the equation for a third reaction. Use a calorimeter to measure the temperature change in each of three reactions. Calculate the heat of reaction, H, for the three reactions. Use the results to confirm Hess’s law.
- 4. LabQuest 18 18 - 2 Chemistry with Vernier MATERIALS LabQuest 4.00 g of solid NaOH LabQuest App ring stand Temperature Probe utility clamp 50 mL of 1.0 M NaOH stirring rod 50 mL of 1.0 M HCl Styrofoam cup 100 mL of 0.50 M HCl 250 mL beaker 100 mL of water PROCEDURE Reaction 1
- 5. 1. Obtain and wear goggles. 2. Connect the Temperature Probe to LabQuest and choose New from the File menu. If you have an older sensor that does not auto-ID, manually set up the sensor. 3. Use a utility clamp to suspend a Temperature Probe from a ring stand as shown in Figure 1. 4. Place a Styrofoam cup into a 250 mL beaker as shown in Figure 1. Measure out 100.0 mL of water into the Styrofoam cup. Lower the Temperature Probe into the solution. 5. CAUTION: Handle the NaOH and resulting solution with care. Weigh out about 2 g of solid sodium hydroxide, NaOH, and record the mass to the nearest 0.01 g. Note: NaOH(s) is highly hygroscopic; it readily absorbs moisture from the surrounding environment. This additional water weight is not negligible and can directly impact your results. Make sure to weigh your solid NaOH quickly and proceed to the next step without delay. Please take care to keep the
- 6. solid NaOH jar sealed when not in use. NaOH(s) that has been exposed to too much moisture will appear wet and shiny. Ask your TA to inspect the NaOH(s) is you are unsure. 6. Start data collection and obtain the initial temperature, t1. Monitor temperature (in °C) on the screen. It may take several seconds for the Temperature Probe to equilibrate at the temperature of the solution. After three or four readings at the same temperature have been obtained, add the solid NaOH to the Styrofoam cup. Using the stirring rod, stir continuously until the temperature has maximized and then begun to drop. At this point, all reactant has been consumed and your open-calorimeter system is losing heat to the surrounding environment. Record the maximum temperature, t2, before the drop in temperature occurred. 7. Data collection will stop after 3 minutes. You can manually stop data collection if your temperature peak and drop occurs before 3 minutes has elapsed. Conversely, if your peak needs longer than 3 minutes, you can adjust the LabQuest to
- 7. record data for longer than the default 180 seconds. 8. To confirm the initial (t1) and final (t2) values you recorded earlier, examine the data points along the curve on the displayed graph. As you tap each point, the temperature and time values are displayed to the right of the graph. Figure 1 Additivity of Heats of Reaction: Hess’s Law Chemistry with Vernier 18 - 3 9. Rinse and dry the Temperature Probe, Styrofoam cup, and stirring rod. Dispose of the solution in the aqueous waste bin. Ask your TA for its location. Reaction 2 10. CAUTION: Handle the HCl solution and NaOH solid with care. Repeat Steps 4–9, using
- 8. 100.0 mL of 0.50 M hydrochloric acid, HCl, instead of water. Use the same amount of solid NaOH as before. Reaction 3 11. CAUTION: Handle the HCl and NaOH solutions with care. Repeat Steps 4–9, initially measuring out 50.0 mL of 1.0 M HCl (instead of water) into the Styrofoam calorimeter. In Step 5, instead of solid NaOH, measure 50.0 mL of 1.0 M NaOH solution into a graduated cylinder. After 3–4 temperature readings have been taken to determine the initial temperature of the 1.0 M HCl, add the 1.0 M NaOH solution to the Styrofoam cup. PROCESSING THE DATA 1. Determine the mass of 100 mL of solution for each reaction (assume the density of each solution is 1.00 g/mL). 2. Determine the temperature change, t, for each reaction.
- 9. 3. Calculate the heat released by each reaction, q, by using the formula: q = Cp•m• t (Cp = 4.18 J/g°C) Convert joules to kJ in your final answer. 4. Find H ( H = –q ). 5. Calculate moles of NaOH used in each reaction. In Reactions 1 and 2, this can be found from the mass of the NaOH. In Reaction 3, it can be found using the molarity, M, of the NaOH and its volume, in L. 6. Use the results of the Step 4 and Step 5 calculations to determine H/mol NaOH in each of the three reactions. 7. To verify the results of the experiment, combine the heat of reaction ( H/mol) for Reaction 1 and Reaction 3. This sum should be similar to the heat of reaction ( H/mol) for Reaction 2. Using the value in Reaction 2 as the accepted value and the sum of Reactions 1 and 3 as the
- 10. experimental value, find the percent error for the experiment. LabQuest 18 18 - 4 Chemistry with Vernier DATA AND CALCULATIONS Reaction 1 Reaction 2 Reaction 3 1. Mass of solid NaOH g g (no solid NaOH mass) 2. Mass (total) of solution g
- 11. g g 3. Final temperature, t2 °C °C °C 4. Initial temperature, t1 °C
- 12. °C °C 5. Change in temperature, t °C °C °C 6. Heat, q kJ
- 13. kJ kJ 7. H kJ kJ kJ 8. Moles of NaOH mol mol
- 14. mol 9. H/mol kJ/mol kJ/mol kJ/mol 10. Experimental value kJ/mol 11. Accepted value kJ/mol 12. Percent error % , lllll ALL 102 ALL
- 18. -5260.8 ALL -4433.71 ALL 7.23 Additivity of Heats of Reaction: Hess’s Law Chemistry with Vernier 18 - 5 KEY LEARNING POINTS balancing reactions calorimeter/calorimetry Hess’s law heat (enthalpy) of reaction specific heat q = mC∆T