The specific heat (C) is the quantity of heat required to raise the temperature of one gram of a substance by one degree Celsius or Kelvin. A calorimeter constant is a constant that measures the heat capacity of the calorimeter. It is calculated by applying a known amount of the heat and determining the resultant change in temperature in the calorimeter
Determination of enthalpy of ionisation of acetic acidMithil Fal Desai
The acetic acid is a weak acid as it does not completely dissociate in dilute aqueous solutions into hydrogen (H+) and acetate (CH3COO-) ions. When acetic acid is neutralized with a strong base (NaOH), heat is evolved during the neutralization that is used in the process of dissociating the acetic acid further that will facilitate the completion of neutralization.
CH3COOH + NaOH = CH3COONa + H2O + heat
The enthalpy change associated with the neutralization of acetic acid with a strong base is lower than that of the enthalpy of neutralization of a strong acid with a strong base. The difference in the enthalpy of neutralization of a strong acid (HCI) with a strong base (NaOH) and enthalpy of neutralization of weak acid (CH3COOH) with a strong base (NaOH) is the enthalpy of ionization of the weak acid (CH3COOH).
DETERMINATION OF THE EQUILIBRIUM CONSTANT FOR THE FORMATION OF TRI-IODIDE IONAugustine Adu
A LABORATORY WORK THAT WILL HELP ANYONE TO DETERMINE EQUILIBRIUM CONSTANT OF TRI-IODIDE ION.
THE EQUILIBRIUM CONSTANT IS NOT DIRECTLY DETERMINED, THIS PIECE WILL GIVE A WAY TO HOW IT IS DONE.
The specific heat (C) is the quantity of heat required to raise the temperature of one gram of a substance by one degree Celsius or Kelvin. A calorimeter constant is a constant that measures the heat capacity of the calorimeter. It is calculated by applying a known amount of the heat and determining the resultant change in temperature in the calorimeter
Determination of enthalpy of ionisation of acetic acidMithil Fal Desai
The acetic acid is a weak acid as it does not completely dissociate in dilute aqueous solutions into hydrogen (H+) and acetate (CH3COO-) ions. When acetic acid is neutralized with a strong base (NaOH), heat is evolved during the neutralization that is used in the process of dissociating the acetic acid further that will facilitate the completion of neutralization.
CH3COOH + NaOH = CH3COONa + H2O + heat
The enthalpy change associated with the neutralization of acetic acid with a strong base is lower than that of the enthalpy of neutralization of a strong acid with a strong base. The difference in the enthalpy of neutralization of a strong acid (HCI) with a strong base (NaOH) and enthalpy of neutralization of weak acid (CH3COOH) with a strong base (NaOH) is the enthalpy of ionization of the weak acid (CH3COOH).
DETERMINATION OF THE EQUILIBRIUM CONSTANT FOR THE FORMATION OF TRI-IODIDE IONAugustine Adu
A LABORATORY WORK THAT WILL HELP ANYONE TO DETERMINE EQUILIBRIUM CONSTANT OF TRI-IODIDE ION.
THE EQUILIBRIUM CONSTANT IS NOT DIRECTLY DETERMINED, THIS PIECE WILL GIVE A WAY TO HOW IT IS DONE.
Aim: Estimate the amount of Nickel present in a given solution as bis(dimethy...Mithil Fal Desai
Nickel(II) reacts with dimethylglyoxime [C4H6(NOH)2] to form a neutral coordination complex. The formation of the red chelate occurs quantitatively in an aqueous solution at pH 5 to 9. Usually, citric acid is added to lower the interference of other ions like iron.
Determination of the molecular weight of high polyvinyl alcohol (pva) by visc...PRAVIN SINGARE
This presentation is based on demonstration on the Determination of the molecular weight of high polyvinyl alcohol (pva) by viscosity method. The presentation is made for Undergraduate Chemistry Students of Mumbai University
Synthesis of tris (thiourea) copper (i) sulphate by kwezi mwaka juliusMakerere University
its a well described report on SYNTHESIS OF TRIS (THIOUREA) COPPER (I) SULPHATE and this serves to industrial chemistry students doing transition metal chemistry.
Determine the composition of the fe3+(jobs method)Mithil Fal Desai
In Job's method, the variation in concentration of the reactants is performed which can reveal the empirical formula of a complex. The method is employed to find the formula of the compound formed by reacting two or more chemical species. The absorption is recorded against different wavelengths and wavelength having maximum absorption is selected. The intensity of solutions with different stoichiometric ratios of the reactants is measured. The highest observed intensity reveals the maximum amount of compound formed. In this experiment, the Fe3+ and salicylic acid are reacted and the wavelength at which the complex absorbs strongly is selected. The absorbance of the different stoichiometric ration of Fe3+ and salicylic acid at a selected wavelength is determined. The maximum absorbance of the solution of the stoichiometric ratio reveals the empirical formula of the complex as the maximum amount of coloured complex is formed.
INTRODUCTIONChemical reactions are generally accompanied by some.docxnormanibarber20063
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.
Aim: Estimate the amount of Nickel present in a given solution as bis(dimethy...Mithil Fal Desai
Nickel(II) reacts with dimethylglyoxime [C4H6(NOH)2] to form a neutral coordination complex. The formation of the red chelate occurs quantitatively in an aqueous solution at pH 5 to 9. Usually, citric acid is added to lower the interference of other ions like iron.
Determination of the molecular weight of high polyvinyl alcohol (pva) by visc...PRAVIN SINGARE
This presentation is based on demonstration on the Determination of the molecular weight of high polyvinyl alcohol (pva) by viscosity method. The presentation is made for Undergraduate Chemistry Students of Mumbai University
Synthesis of tris (thiourea) copper (i) sulphate by kwezi mwaka juliusMakerere University
its a well described report on SYNTHESIS OF TRIS (THIOUREA) COPPER (I) SULPHATE and this serves to industrial chemistry students doing transition metal chemistry.
Determine the composition of the fe3+(jobs method)Mithil Fal Desai
In Job's method, the variation in concentration of the reactants is performed which can reveal the empirical formula of a complex. The method is employed to find the formula of the compound formed by reacting two or more chemical species. The absorption is recorded against different wavelengths and wavelength having maximum absorption is selected. The intensity of solutions with different stoichiometric ratios of the reactants is measured. The highest observed intensity reveals the maximum amount of compound formed. In this experiment, the Fe3+ and salicylic acid are reacted and the wavelength at which the complex absorbs strongly is selected. The absorbance of the different stoichiometric ration of Fe3+ and salicylic acid at a selected wavelength is determined. The maximum absorbance of the solution of the stoichiometric ratio reveals the empirical formula of the complex as the maximum amount of coloured complex is formed.
INTRODUCTIONChemical reactions are generally accompanied by some.docxnormanibarber20063
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.
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 ...
LabQuest 18 Chemistry with Vernier 18 - 1 Additi.docxMARRY7
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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The dissolved strong mineral acids, weak organic acids, dissolved carbon dioxide and hydrolyzed mineral salts may contribute to the measured acidity of natural water. The acidity of water is a significant parameter of water as the presence of acids in natural water contributes to corrosiveness and influences chemical reaction rates. The biological processes are dependent on the acidity of water. The quantitative acidity measurement also reflects the quality of the source of water. The acidity of water is usually expressed in terms of CaCO3.
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Artificial Intelligence (AI) technologies such as Generative AI, Image Generators and Large Language Models have had a dramatic impact on teaching, learning and assessment over the past 18 months. The most immediate threat AI posed was to Academic Integrity with Higher Education Institutes (HEIs) focusing their efforts on combating the use of GenAI in assessment. Guidelines were developed for staff and students, policies put in place too. Innovative educators have forged paths in the use of Generative AI for teaching, learning and assessments leading to pockets of transformation springing up across HEIs, often with little or no top-down guidance, support or direction.
This Gasta posits a strategic approach to integrating AI into HEIs to prepare staff, students and the curriculum for an evolving world and workplace. We will highlight the advantages of working with these technologies beyond the realm of teaching, learning and assessment by considering prompt engineering skills, industry impact, curriculum changes, and the need for staff upskilling. In contrast, not engaging strategically with Generative AI poses risks, including falling behind peers, missed opportunities and failing to ensure our graduates remain employable. The rapid evolution of AI technologies necessitates a proactive and strategic approach if we are to remain relevant.
Determination of enthalpy of neutralization of hydrochloric acid with sodium hydroxide
1. SHREE MALLIKARJUN COLLEGE CLASS:FYBSC
SAFETY: Refer to the MSDS of of hydrochloric acid and sodium hydroxide.
-Dr. Mithil S. FalDesai
Aim: Determination of enthalpy of neutralization of hydrochloric acid with sodium hydroxide.
Chemicals: HCl, NaOH
Apparatus/Instrument: Beaker, measuring cylinder, thermometer, calorimeter
Theory: The heat of neutralization is heat produced when 1 mole of water is produced by the
reaction of the acid and base. One mole of HCl reacts with one mole of NaOH to give one mole
of water.
HCl + NaOH NaCl + H2O + heat
Above reaction is done in a calorimeter whose heat capacity (Ccal) is previously determined or
known. The heat change during the neutralization is measured using a thermometer. Change in
temperature after mixing acid and base is given by
Δt = T2-T1 --------------eq 1
Thus, heat gained by the calorimeter is equal to the heat of neutralization (qneutralization).
qneutralization = Ccal XΔt --------------eq 2
The enthalpy of neutralization (ΔH) is given by
ΔH = (qneutralization)/ Number of moles of water formed --------------eq 3
The unit of enthalpy is J mol-1.
Procedure:
1) Take 50 ml of 2.0 M HCl and 50 mL of 2.0 M NaOH in two beakers; wait for 30 min so that a
solution attains the room temperature.
2) Measure the temperature of both the solutions (T1).
3) Pour 50 ml of 2.0 M HCl in the calorimeter.
4) Add quickly 50 ml of 2.0 M NaOH and stir.
5) Note down the maximum temperature of the resultant solution attained after the mixing (T2).
Result: The enthalpy of neutralization of hydrochloric acid with sodium hydroxide =___ J mol-1.
Questions
1) What is enthalpy?
2) What is heat capacity of calorimeter?
3) Compare the enthalpy of neutralization of acetic acid and hydrochloric acid.
4) What is a calorimeter and colorimeter?
5) Why usually water is used for calorimetric measurments?
2. SHREE MALLIKARJUN COLLEGE CLASS:FYBSC
SAFETY: Refer to the MSDS of of hydrochloric acid and sodium hydroxide.
-Dr. Mithil S. FalDesai
