1. Understand that Energy is exchanged or transformed in all chemical reactions and physical changes of matter. As a basis for understanding this concept: (a) Students know how to describe temperature and heat flow in terms of the motion of molecules (or atoms) and (b) Students know chemical processes can either release (exothermic) or absorb (endothermic) thermal energy.
Basic Terminology,Heat, energy and work, Internal Energy (E or U),First Law of Thermodynamics, Enthalpy,Molar heat capacity, Heat capacity,Specific heat capacity,Enthalpies of Reactions,Hess’s Law of constant heat summation,Born–Haber Cycle,Lattice energy,Second law of thermodynamics, Gibbs free energy(ΔG),Bond Energies,Efficiency of a heat engine
In this PPT have have covered
1. Basic thermodynamics definition
2. Thermodynamics law
3. Properties , cycle, Process
4. Derivation of the Process
5.Formula for the numericals.
This topic is use full for those students who want to study basic thermodynamics as a part of their University syllabus.
Most of the university having basic Mechanical engineering as a subject and in this subject Thermodynamics is a topic so by this PPT our aim is to give presentable knowledge of the subject
The following presentation consists of information on limitation of 1st law, introduction to 2nd law, kelvin planks statement, Clausius statement, PPM 2, Carnot cycle, Carnot heat engines, etc
thermodynamics, basic definitions with explanations, heat transfer, mode of heat transfer, Difference between thermodynamics and heat transfer?What is entropy?
Introduction to the second law
Thermal energy reservoirs
Heat engines
Thermal efficiency
The 2nd law: Kelvin-Planck statement
Refrigerators and heat pumps
Coefficient of performance (COP)
The 2nd law: Clasius statement
Perpetual motion machines
Reversible and irreversible processes
Irreversibility's, Internal and externally reversible processes
The Carnot cycle
The reversed Carnot cycle
The Carnot principles
The thermodynamic temperature scale
The Carnot heat engine
The quality of energy
The Carnot refrigerator and heat pump
Basic Terminology,Heat, energy and work, Internal Energy (E or U),First Law of Thermodynamics, Enthalpy,Molar heat capacity, Heat capacity,Specific heat capacity,Enthalpies of Reactions,Hess’s Law of constant heat summation,Born–Haber Cycle,Lattice energy,Second law of thermodynamics, Gibbs free energy(ΔG),Bond Energies,Efficiency of a heat engine
In this PPT have have covered
1. Basic thermodynamics definition
2. Thermodynamics law
3. Properties , cycle, Process
4. Derivation of the Process
5.Formula for the numericals.
This topic is use full for those students who want to study basic thermodynamics as a part of their University syllabus.
Most of the university having basic Mechanical engineering as a subject and in this subject Thermodynamics is a topic so by this PPT our aim is to give presentable knowledge of the subject
The following presentation consists of information on limitation of 1st law, introduction to 2nd law, kelvin planks statement, Clausius statement, PPM 2, Carnot cycle, Carnot heat engines, etc
thermodynamics, basic definitions with explanations, heat transfer, mode of heat transfer, Difference between thermodynamics and heat transfer?What is entropy?
Introduction to the second law
Thermal energy reservoirs
Heat engines
Thermal efficiency
The 2nd law: Kelvin-Planck statement
Refrigerators and heat pumps
Coefficient of performance (COP)
The 2nd law: Clasius statement
Perpetual motion machines
Reversible and irreversible processes
Irreversibility's, Internal and externally reversible processes
The Carnot cycle
The reversed Carnot cycle
The Carnot principles
The thermodynamic temperature scale
The Carnot heat engine
The quality of energy
The Carnot refrigerator and heat pump
The chemical energy of a system is changed as a result of a reaction. Calorimetry. Heat of combustion . Calculation of caloric content of sucrose or food. Combustion reaction.
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 ...
What is the tool used to measure the heat absorbed or released. What is the difference between heat and enthalpy. What happen in an endothermic and exothermic reactions.
Exploiting Artificial Intelligence for Empowering Researchers and Faculty, In...Dr. Vinod Kumar Kanvaria
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Knowledge and skills frameworks, generally called competency frameworks, for ELT teachers, trainers and managers have existed for a few years now. However, until I created one for my MA dissertation, there wasn’t one drawing together what we need to know and do to be able to effectively produce language learning materials.
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• The Committee on Ways and Means has been investigating several universities since November 15, 2023, when the Committee held a hearing entitled From Ivory Towers to Dark Corners: Investigating the Nexus Between Antisemitism, Tax-Exempt Universities, and Terror Financing. The Committee followed the hearing with letters to those institutions on January 10, 202
Embracing GenAI - A Strategic ImperativePeter Windle
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.
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BÀI TẬP BỔ TRỢ TIẾNG ANH GLOBAL SUCCESS LỚP 3 - CẢ NĂM (CÓ FILE NGHE VÀ ĐÁP Á...
What is enthalpy
1. What is Enthalpy?
Author: Dr. Robert D. Craig, Ph.D
Day 13
This lesson and Laboratroy procedure was adapted from
http://chemistry.allinfoabout.com/features/calorimeter.htm
by Dr. Anne Helmenstine
and
Physical properties of matter by Carl Martiken
http://www.iit.edu/~smart/martcar/lesson5/id37.htm
The problem set was developed by S.E. Van Bramer for Chemistry 145 at Widener
University and the 1997 regents Exam
Aim: What is Enthalpy?
IO/SWBAT :
1. Understand that Energy is exchanged or transformed in all chemical
reactions and physical changes of matter. As a basis for understanding this
concept: (a) Students know how to describe temperature and heat flow in
terms of the motion of molecules (or atoms) and (b) Students know
chemical processes can either release (exothermic) or absorb
(endothermic) thermal energy.
CONTENT STANDARD: (THE PHYSICAL SETTING)
www.nysed.gov
1. Chemical and physical changes can be exothermic or endothermic (4.1b)
2. Distinguish between endothermic and exothermic reactions, using energy
terms in a reaction equation, ∆H, potential energy diagrams or
experimental data (4.1i)
PROCESS STANDARDS:
http://www.emsc.nysed.gov/ciai/mst/sciencestand/physset13.html
http://www.emsc.nysed.gov/ciai/mst/sciencestand/physset45.htm l
Standard 1: Analysis, Inquiry and Design
Mathematical Analysis
2. Students will use mathematical analysis to calculate the heat involved in a phase or
temperature change for a given sample of matter (4.2iv)
Standard 4: Science
develop their own mental models to explain common chemical reactions and changes in
states
Motivation: How to measure heat flow and enthalpy change using a Coffee Cup
Bomb Calorimetry ?
Lesson:
The term enthalpy is composed of the prefix en-, meaning to "put into", plus the Greek
word -thalpein, meaning "to heat",
It is often calculated as a differential sum, describing the changes within exo- and
endothermic reactions, which minimize at equilibrium Enthalpy change is defined by the
following equation:
Where,
ΔH is the enthalpy change
Hfinal is the final enthalpy of the system, measured in joules. In a chemical reaction,
Hfinal is the enthalpy of the products.
Hinitial is the initial enthalpy of the system, measured in joules. In a chemical reaction,
Hinitial is the enthalpy of the reactants.
The Bomb Calorimeter
A calorimeter is a device that is used to measure the quantity of heat flow in a chemical
reaction. Two common types of calorimeters are the coffee cup calorimeter and the bomb
calorimeter the devise has an outer insulated portion which is viewed as the end of the
universe—no heat or work can pass it. The contents of the outer insulated container
consists of the stell “bomb”, a sample dish within the “bomb”, ignition wires into the
“bomb” and touching the chemical sample dish, water surrounding the “bomb”, a stirrer,
and a thermometer. The contents of the “bomb” are the system and the other contents of
insulate container (including the walls of the “bomb”) are the surroundings. The wall of
the “bomb” is the boundary. The “bomb” confines the system to constant volume.
3. From the law of conservation of energy, we can deduce that
The heat transferred from the system = the heat transferred into the surrounding the left
term is just the heat of the reaction (qv) and the right term is the sum of the heat absorbed
by the water and the heat absorbed by the bomb’s stainless steel walls so we have
-qv = q water + q bomb
Where the negative sign is required because heat is lost from the system (exothermic)
To determine the above we will need the individual values:
Q water = mass of water*(specific heat of water)*(∆T) and
Q bomb = heat capacity of bomb * ∆T
The heat capacity of the bomb is determined by first doing an experiment with some
chemical for which you know the heat of combustion so that you can solve the equations
for the heat capacity of the bomb. Then the unknown is run using the previously
determined value for the heat capacity of the bomb.
Procedure:
The coffee Cup Calorimeter
Students will begin experiment by Carl Martiken
http://www.iit.edu/~smart/martcar/lesson5/id37.htm
Back ground Information:
A coffee cup calorimeter is essentially a polystyrene (Styrofoam) cup with a lid.
Really, any well-insulated container will work. The cup is partially filled with a known
volume of water and a thermometer is inserted through the lid of the cup so that the
thermometer is inserted through the lid of cup so that the thermometer bulb is below the
surface. The water absorbs the heat of any chemical reaction taking place in the
4. calorimeter. The change in the water temperature is used to calculate the amount of heat
that has been absorbed.
Heat flow is calculated using the relation:
Q = (specific heat) x m x ∆T
Where q is heat flow, m is mass in grams, and ∆T is the change in temperature. The
specific heat is the amount of heat required to raise the temperature of 1 gram of a
substance 1 degree Celcius. The specific heat of (pure) water is 4.18 J/(g.oC)
For example, consider a chemical reaction which occurs in 200 grams of water with an
initial temperature of 25.0 oC. The reaction is allowed to proceed in the coffee cup
calorimeter. As a result of the reaction, the temperature of the water changes to 31.0C.
the heat flow is calculated:
q water = 4.18 j/(g.oC) x 200 g x (31.0 oC -25.0 oC)
q water = +5.0 x 103 J
In other words, the products of the reaction evolved 5000 J of heat, which was lost to the
water. The enthalpy change, ∆ H, for the reaction is equal in magnitude by opposite to
the heat flow for the water
∆ H reaction = - (q water)
For an exothermic reaction, ∆H < 0; q water is positive. The water absorbs heat from the
reaction and an increase in temperature is seen. For an endothermic reaction, ∆H > 0; q
water is negative. The water supplies heat for the reaction and a decrease in temperature
is seen
A coffee cup calorimeter is great for measuring heat flow in a solution, but it can’t be
used for reactions which involve gases, since they would escape from the cup. Also, a
coffee cup calorimeter can’t be used for high temperature reactions, since high heat
would meld the cup. A bomb calorimeter is used to measure heat flows for gases and
high temperature reactions.
‘
A bomb calorimeter works the same way as a coffee cup calorimeter, with one big
difference. In a coffee cup calorimeter, the reaction takes place in the water. In a bomb
calorimeter, the reaction takes place in a sealed metal container, which is placed in the
water in an insulated container. Heat flow from the reaction crosses the walls of the
sealed container to the water. The temperature difference of the water is measured, just
as it was for a coffee cup calorimeter.
5. Analysis of the heat flow is a bit more complex than it was for the coffee cup calorimeter
because the heat flow into the metal parts of the calorimeter must be taken into account:
q reaction = -(q water + q bomb)
Where q water = 4.18 J/ (g. oC)) x mwater x ∆T
The bomb has a fixed mass and specific heat. The mass of the bomb multiplied by its
specific heat is sometimes termed the calorimeter constant, denoted by the symbol C with
units of joules per degree Celsius. The calorimeter constant, denoted by the symbol C
with units of joules per degree Celsius. The calorimeter constant is determined
experimentally and will vary from one calorimeter to the next. The heat flow of the
bomb is:
q bomb = C x ∆T
Once the calorimeter constant is known, calculating heat flow is a simple matter. The
pressure within a bomb calorimeter often changes during a reaction, so the heat flow may
not be equal in magnitude to the enthalpy change.
6. Energy and Enthalpy Homework Problem Set
This problem set was developed by S.E. Van Bramer for Chemistry 145 at Widener University.
1. What occurs when the temperature of 10.0 grams of water (June ’93) is changed
from 15.5 oC to 14.5 oC
a. The water absorbs 10.0 calories
b. The Water releases 10.0 calories
c. The water absorbs 155 calories
d. The water releases 145 calories
2. A piece of titanium metal (mass 452.398 g) is placed in boiling water (100.00 °C).
After 20 minutes it is removed from the boiling water and placed in a 1.000 liter
container of water at 20.00 °C. The temperature of the water increases to 24.28 °C.
What is the specific heat of titanium?
3. Next the same piece of titanium is heated in acetylene flame (like that used for
welding) to an unknown temperature. When the pieced of titanium is placed in a
10.000 liter container of water at 20.00 oC the final temperature is now 30.72 oC.
What is the temperature of the flame? At what temperature does titanium melt?
4. Calculate the energy required to heat a 155.4 g ice cube that starts in a freezer at
-100.0 °C (VERY COLD):
a. Heat from the freezer to ice at 0.0 °C.
b. Heat from ice at 0.0 °C to liquid at 0.0°C.
c. Heat from liquid at 0.0 °C to liquid at 100.0 °C.
d. Heat from liquid at 100.0 °C to gas at 100.0 °C.
e. Heat from gas at 100.0 °C to gas at 200.0 °C.