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CE CH. 8 REVIEW RXN RATES & EQUILIBRIUM - write on … CH. 8 REVIEW RXN RATES & EQUILIBRIUM - write on your own paper Definitions: 1. Activation Energy 2. Catalytic Action or Catalyst

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Page 1: CE CH. 8 REVIEW RXN RATES & EQUILIBRIUM - write on … CH. 8 REVIEW RXN RATES & EQUILIBRIUM - write on your own paper Definitions: 1. Activation Energy 2. Catalytic Action or Catalyst

CE CH. 8 REVIEW RXN RATES & EQUILIBRIUM - write on your own paper

Definitions:

1. Activation Energy

2. Catalytic Action or Catalyst

3. Endergonic

4. Energy

5. Entropy

6. Exergonic system loses energy

7. Inhibitor

8. Nonspontaneous process

9. Reaction rate

10. Spontaneous process

11. If a solid spontaneously sublimes to a gas. What happens to the entropy? What happens to the

energy? Energy & entropy increase

12. Write the states of matter in order of increasing entropy. Solid < liquid< gas

13. What conditions are necessary for a chemical reaction to occur? The molecules of the reacting chemicals must bump into each other.

14. What conditions are necessary for a spontaneous reaction?

The reaction proceeds without needing continuous input

15. For a reaction to happen, what conditions must be present? Particles must collide with enough energy and the

correct orientation

16. How can activation energy be lowered? Use a catalyst

17. What are the factors that influence the rate of a reaction? Temperature, surface area of particles, and concentration of reactants

18. Describe how a catalyst works. A catalyst lowers the activation energy

19. How do homogeneous catalysts work? A catalyst lowers the activation energy 20. Explain how a catalyst affects the equilibrium position. A catalyst does not have any affect on the equilibrium

position. 21. For the reaction A + B C , describe what happens to the concentrations of each reactant and product once

pure A and B are mixed together? The concentrations of A & B decrease and the concentration of C increases The following 2 questions refer to the equilibrium given below in which all reactants and products are gases.

CH4 + H2O CH3OH + H2 + heat

22. Write the equation for the equilibrium constant for the equation. 𝐾𝑒𝑞 = [𝐶𝐻3OH][𝐻2]

[𝐶𝐻4][𝐻2𝑂]

23. Indicate the effect of the changing condition on the position of equilibrium. a. Add CH4 to the mixture. To right b. Remove H2 from the mixture. to right

c. Cool the mixture. to right d. Add a catalyst to the mixture. none

24. Write the equilibrium expression for the reaction N2 + 3H2 2NH3 𝐾𝑒𝑞 = [𝑁𝐻3]2

[𝑁2] [𝐻2]3

25. BrCl is put into an empty 1.00 L container. At equilibrium, the molar concentration of BrCl is 0.382, and that of Br2= Cl2 =0.319. Evaluate the equilibrium constant for the following reaction. Br2(g) + Cl2(g) 2BrCl(g)

𝐾𝑒𝑞 = [0.382]2

[0.319] [0.319] = 1.43

26. TRUE or FALSE: If the reaction A + B C is exothermic, the concentration of C should increase with increasing temperature.

27. TRUE or FALSE: The reaction represented by this energy diagram is endothermic. 28.

28. TRUE or FALSE: The only way to increase the rate of a reaction is to increase the concentration of the reactants.

29. TRUE or FALSE: For the reaction NO2 (g) + N2O(g) 3 NO(g) the equilibrium constant expression is:

30.

30. What is the direct cause of a chemical reaction of the type E + F EF? Effective collisions need to occur between E & F

31. How does the rate of the reverse reaction compare to the rate of the forward reaction when a system is at equilibrium? At equilibrium the rate of the forward and reverse reaction are equal.

Page 2: CE CH. 8 REVIEW RXN RATES & EQUILIBRIUM - write on … CH. 8 REVIEW RXN RATES & EQUILIBRIUM - write on your own paper Definitions: 1. Activation Energy 2. Catalytic Action or Catalyst

32. Describe the difference between a large K value compared to a small K value in general for equilibria. A large K value tells us that there are more products than reactants at equilibrium. A small K value means that there are more reactants than products at equilibrium.

33. If we remove CO2 from the following equation, which way will the equilibrium shift? CO + H2O + heat CO2 + H2 to right

34. If we add a catalyst to the following equation, which way will the equilibrium shift?

CO + H2O + heat CO2 + H2 no change in the equilibrium position 35. What would be the effect of doubling the pressure on the following equilibrium system?

N2(g) + 3F2(g) 2NF3(g) to right

36. Write the equilibrium expression for the system N2(g) + 3F2(g) 2NF3(g) 𝐾𝑒𝑞 = [𝑁𝐹3]2

[𝑁2] [𝐹2]3

37. For the following reaction, which of the given changes will increase the value of the equilibrium constant?

AB + CD AD + BC + heat

a. Decreasing the temperature

b. Adding AB to the reaction

c. Removing CD from the reaction

d. All of the changes will increase K 38.

38. For the following energy diagram, which letter represents the catalyzed activation

energy? Also, indicate which of the reactions is exothermic which is endothermic.

C, both reactions are exothermic 39.

39. Consider the following energy diagram. Which letter represents the activation energy

for the forward reaction?

40. Based upon the energy diagram given below, which

letter represents the enthalpy for the reaction? B

41. A room filled with a 2:1 mixture of hydrogen and oxygen gases with a single spark, it can react explosively. Since

the explosion would be considered a spontaneous process, what did the spark provide? The activation energy

42. How can you use the equilibrium constant value to predict if a reaction goes to completion or has more reactants or more products? If the k value is very large (1036) then the reaction is considered to go to completion. If the K value is close to 1, then there are about equal amount of reactants and products. If K is less then 1 there are more reactants than products.

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