Subject: Heat in chemical reactions
Topic:Chemical reactions that involve heat transfer
Grade Level: 11
Student Lesson name and URL: Heat and Thermochemistry

Chemical Thermodynamics 7.(a-d)
7. 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).
b. Students know chemical processes can either release (exothermic) or absorb (endothermic) thermal energy.
c. Students know energy is released when a material condenses or freezes and is absorbed when a material evaporates or melts.
d. students know how to solve problems involving heat flow and temperature changes, using known values of specific heat and latent heat of phase change.
 

Eleventh Grade
Science: Focus on Heat Transfer

Student Activities
  Pretest on heat
           Interpret pictures on web pages
           Warm-up questions on heat
           Video tape on heat application and questions
           Demonstration and questions
           Read and take notes from textbook and articles from the internet
           Lecture on heat 
           Worksheet in class and homework
           Lab activities and report
           Quizzes and test

Student Page

Introductory Activities

DAY 1
Exothermic and Endothermic reactions
Demonstration of Reations I and II:
I. Exothermic reaction: sugar and concentrated sulphuric acid
   (Instruction from Demo Book #38)
II. Endothermic reaction: ammonium hydroxide in water
    (Instruction Demo Book #39))
Questions:
1. What are the temperature changes for reaction I and II? 
    Which one gets hotter and which one gets colder?
2.  For  exothermic reaction and endothermic reactions:
     a. What happens to the temperatures of the environment before and after the reaction?
     b. Does energy get absorbed or released into the environment?
3.Where does the energy come from and go to for each reaction?

DAY 2
Heat and Temperature
Pictures
Questions:
1. What is happening in each of the photographs?
2. Which one is showing energy being produced and/or energy being  consumed?
3.  What happens to temperature changes?
4. What are some other processes that produce energy in the form of heat?
5. Where does the energy come from in each picture?

Day 3
Evaporation
Drop a few drops of water on the back of the hand and let them dry off. Do you feel hot or cold? What type of reaction is this? How does the heat energy transfer?

Day 4 
Warm Up Questions on Exothermic and Endothermic Reactions.
Enthalpy and Heating Fuels: Compare the economical values of propane and methane gases. (Prentice Hall Workbook 12-1 Apply).

Day 5
Warm up questions on heat capacity and specific heat

Day 6 to 9
Warm up questions or demonstrations

Day 10
Review

Enabling Activity(ies)

DAY 1

A. Pretest: Work on Pretest
B. Lecture on Exothermic and Endothermic reactions.
C. Exodermic and endothermic Changes exercise
     Chemistry (Prentice Hall) Chapter 12:Heat in Chemical  Reaction Workbook P. 8:12-1 Apply (Classwork and homework). Use textbook as reference.
 

DAY 2

A. Do lab on Exothermic reaction and Endothermic reaction.
B. Answer questions after each lab.
C. Discussions on endothermic and exothermic reactions.
D. Read Heat and Enthalpy Changes and answer questions.

DAY 3
A. Lecture on Enthalpy(H)  and Enthalpy Change (delata H)
     in exothermic and endothermic reaction.
B. Chemical equations on exothermic and endothermic reactions.
      Work on Equations.
C. Practice Problems #1-10 on Prentice Hall Workbook, 12-2 Practice Problems.
E. Do Chapter 12 Problem Banks #34 to 40

DAY 4
A. Lecture on Total Heat of reaction and Heat of Formation and Calculations.
B. Use standard values of Heat of Formation (deltaH_f^o)(Textbook (Merrill):P.631,Appendix A.Table A-6) to calculate.
C. Do Enthalpy Change Worksheet #3 (on www.google.com:enthalpy change worksheet, page 1, title:Standard Heat of Reaction: Worksheet #3).
D. Reading and questions on Calorimetry.

Day 5
A. Lecture on Calorimetry.
B. Do Ice in Water Lab, discussion on heat and temperature, enthalpy  change.
C. Lecture on specific heat,  heat capacity, and heat exchanges calculations.
D. Do Fire and Ice Lab (Prentice Hall Workbook, 14-4 Explore), and discussion on heat of fusion.

Day 6
1. Review on calorimetry and heat gained=heat lost calculations.
    Use 12-4 Pratice Problem #2 as example
2. Lecture on heat of fusion and phase changes.
3. Lab on finding the latent heat of fusion of ice
   Heat of fusion Lab
4. Discussion on calculations, questions, and lab report format.
5. Finish Lab Report.
5. Do 12-4 Practice Problems #4,6,8,10 and Problem Bank P.409, #45 -48 (Prentice Hall Chemistry Text).

Day 7
Lecture on heat calculations of phase changes.
Enthalpy change of ice from subzero to water to steam. 
Review all  heat calculation problems.
Prelab discussions on Heat of Combustion Lab. Use 'The Chemistry of Burning' Lab Handout.
Homework:
1. Finish all thermochem problems.
2. Write title, objectives, lab procedure, and data table of the Chemistry of Burning Lab'.

Day 8
Heat of Combustion Lab. (Handout)
Calculate Heat of Combustion in KJ/g for paraffin (wax) by burning candles  to heat up water.
Do lab and lab discussion.
Reports to be turned in on Friday.

Day 9
Lecture on Hess's Law
Calculations based on Hess's Law
1. Homework problems on Hess's Law Worksheet
2. Do test review questions #1 to #29
3. Write (Your Own Handwriting, Not Type)
Review Notes

Day 10
Review on endothermic and exothermic reactions, (graphs), 
enthalpy change, standard heat of formation, heat of fusion, heat of combustions, calorimetry: heat lost and heat gained calculations, and Hess's Law.
Review Phase changes of water
Write a brief summary of each of the 5 steps pertaining to changing a piece of ice from subzero temperature to steam.
Click on Phase Change Diagram
a. Draw graph and label the 5 stages.
b. Record data about the piece of ice.
c. Describe what happens to this block of ice at each stage in terms of temperature change, specific heat/ latent heat, and temperature change.
d. Calculate the amount of heat required for the change in each state.
e. Is heat being absorbed or released?
 

DAY 1
1. Exercise on Textbook 12-1 Apply
    a. Study temperature changes of 5 different chemicals dissolving in water.
    b. Classify (endothermic or exothermic)  each reaction.
    c. Explain how energy is being absorbed or released.
2. Do 12-1 Review Questions.

DAY 2
Answer 14 questions based on the reading Heat and Enthalpy Change
A. Transparencies on Mechanism of endothermic and exothermic reactions
Questions: (For each reaction)
1. What is the direction of heat flow? Why?
2. The amount of heat energy in the products is > or < than the reactants?
     Explain why.
3. Temperatures of the environment increases or decrease?.
4. The heat term kJ/J is on the left or right side of the equation?
 

DAY 3
Lab on finding the specific heat of an unknown substance  with given materials.

Day 4 to 10 
Lab Reports and homework assignments

Day 11
Unit Test

IStudents' performance evaluation is based on Homework, Lab reports, and Unit Test.  Check Rubric