1. Chemistry/Physical Setting
Ch. 17 and 18 Review
Br. Jabreal

2. Energy Define three types of energy.
Thermal Energy: Energy associated with random molecular movements
Chemical Energy: Energy associated with bonds
Kinetic Energy: Energy possessed by an objected due to its motion.

3. Practice Which of the following is a unit of energy? Gram Liter Joule
Kilometer

4. Conservation in Chemical Reactions
What are three things conserved in a chemical reaction?

5. What is heat?
Heat:
Energy that transfers from one object to another because of temperature differences
Flows from ________ object to _________ object.
Represented by q.

6. Practice
A laboratory technician takes a test tube of ethanol at 72oC and places it into a beaker containing 150 grams of water at 50oC. The final temperature of the beaker of water and the ethanol reached is 60oC.
State the direction of heat transfer between the beaker and the test tube.
Show a numerical setup for calculating the change in thermal energy of the water.

7. Exothermic vs. Endothermic
What is meant by an exothermic process?
Is heat/energy a product or reactant for exothermic processes?
Give three examples of phase changes that are exothermic.
Which is exothermic: Bond formation of bond breakage?

8. Exothermic vs. Endothermic
What is meant by an endothermic process?
Is heat/energy a product or reactant for endothermic processes?
Give three examples of phase changes that are endothermic.
Which is endothermic: Bond formation of bond breakage?

9. Practice
During photosynthesis, plants use carbon dioxide, water, and light energy to produce glucose, C6H12O6, and oxygen. The reaction for photosynthesis is represented by the balanced equation below.
6CO2 + 6H2O + light energy C6H12O6 + 6O2
State evidence that photosynthesis is an endothermic reaction.

10. Practice

11. Specific Heat Capacity
What is specific heat capacity?
What is the specific heat capacity of water?
How can we calculate energy changes associated with heating a substance up?
q = mCΔT

12. Practice
What is the amount of energy required to raise the temperature of 210 grams of water from 42oC to 50oC?

13. Heat of Fusion What is heat of fusion?
What is the heat of fusion of water?

14. Practice
What is the total amount of heat required to completely melt 347 grams of ice at its melting point?

15. Heat of Vaporization What is heat of vaporization?
What is the heat of vaporization of water?

16. Practice
Show a numerical setup for calculating the quantity of heat in joules required to completely vaporize grams of H2O(ℓ) at 100.°C and 1.0 atm.

17. Heat of Reaction What is the Heat of Reaction (ΔH)?
ΔH = PE(Products) – PE(Reactants)
Which reactions have a positive heat of reaction?
Give two examples
Which reactions have a negative heat of reaction?

18. Practice
How much heat is released when 3 moles of C2H6 form from its elements?

19. Collision Theory Practice
The collision theory states that a reaction is most likely to occur when the reactant particles collide with the proper
(1) Formula masses
(2) Molecular masses
(3) Density and volume
(4) Energy and orientation

20. Practice
Explain, in terms of collision theory, why an increase in temperature increases the rate of a reaction.

21. Practice

22. Collision Theory
Summarize the Collision Theory. What are the requirements for an “effective” collision?
What factors affect the reaction rate?

24. Practice
On the potential energy diagram draw a double-headed arrow to indicate the interval that represents the heat of reaction.

25. Practice
On this diagram, draw a dashed line to show how the potential energy changes when the reaction occurs by the catalyzed pathway.

26. Equilibrium Practice
The equation below represents an equilibrium system of SO2(g), O2(g), and SO3(g).
Compare the rates of the forward and reverse reactions at equilibrium.
State how the equilibrium shifts when SO3(g) is removed from the system.

27. Practice