Unit 13 Review

Kinetics&

Equilibrium

1. Energy that is available to do work is called ____.

A. Exothermic energyB. Endothermic energyC. Gibbs’ Free EnergyD. Heat

2. ____ is defined as the number of atoms, ions, or molecules that react in a given time to form products.

A. Reaction RateB. ConcentrationC. TimeD. Spontaneous Reaction

3. What is the name of the minimum energy that colliding particles must have in order to react?

A. Activated complexB. Activation energyC. Progress of reactionD. Gibb’s Free Energy

4. What is the arrangement of atoms at the peak of an energy barrier?

A. Activated complexB. Activation energyC. ReactantD. Product

5. At equilibrium, what is the rate of production of reactants compared with the rate of production of products?

A. HigherB. LowerC. The sameD. Not enough information

6. The rate of a chemical reaction normally ____ as reactant concentration increases.

A. IncreasesB. DecreasesC. Stays the sameD. Not enough information

7. The amount of disorder in a system is measured by its ____.

A. EnthalpyB. EntropyC. Heat changeD. Gibbs’ Free Energy

8. If a reaction has an equilibrium constant (Keq) just greater than 1, how do we interpret that information?

A. Reactants are favoredB. Products are favoredC. Both reactant and product are favoredD. Neither reactant or product are favored

9. Which variable is NOT required to calculate the Gibbs free-energy change for a chemical reaction?

A. Change in enthalpyB. Change in entropyC. Temperature in oCD. Temperature in K

10. What is the effect of adding more water to the following equilibrium reaction: CO2 + H2O ↔ H2CO3

A. Concentration of H2CO3 decreases

B. Concentration of H2CO3 increases

C. Concentration of CO2 increases

D. Concentration of H2O decreases

11. In an endothermic reaction at equilibrium, what is the effect of raising the temperature?

A. Shift to the reactantsB. Shift to the productsC. No effectD. Not enough information

12. What is the numerical value (+ or -) of Gibbs free-energy change for a spontaneous reaction?

A. ∆G is positiveB. ∆G is negative

13. At what stage of a reaction do atoms have the highest energy?

A. As reactantsB. As productsC. At the transition stage (activated complex)D. They don’t have energy

14. Which of the following systems has the highest entropy:

A. 10 mL of HCl at 50 oC

B. 10 mL of HCl at 100 oC

C. 10 mL of HCl at 75 oC

D. 10 mL of HCl at 10 oC

15. An elementary reaction converts reactants to products in ____.

A. A single stepB. In multiple steps

16. Consider the reaction: N2(g) + 3H2(g) ↔ 2NH3(g)

What is the effect of decreasing the volume on the contained gases?

A. Concentration of NH3 increases

B. Concentration of N2 increases

C. Concentration of H2 decreases

D. Both A and C

17. Spontaneous reactions always ____ free energy.

A. ReleaseB. AbsorbC. ContainD. All of the above

18. What physical state of nitrogen has the highest entropy?

A. SolidB. LiquidC. GasD. All the same

19. What is another name for the catalysts in your body?

A. InhibitorB. DNAC. EnzymeD. RNA

20. In an equilibrium reaction with a Keq of 1 x 108, the ____ are favored.

A. ReactantsB. ProductsC. Both reactants and productsD. Neither reactants or products

21. In which of these systems is the entropy decreasing:

A. Salt dissolving in waterB. A liquid coolingC. Heating a liquidD. Breaking apart a sugar cube

22. In a two-step reaction mechanism, how many elementary reactions occur?

A. 0B. 1C. 2D. 3

23. The Keq of a reaction is 4 x 10-7. At equilibrium, the ____ are favored.

A. reactantsB. productsC. Both reactants and productsD. Neither reactants or products

24. Another name for the activated complex is ____.

A. Activation energyB. reactantC. productD. Transition state

25. A catalyst works by ____.

A. Increasing the amount of energy you need.B. Decreasing the activation energy.C. Acting as an inhibitor.D. None of the above.

Answers

1.C 9. C 17. A2.A 10. B 18. C3.B 11. B 19. C4.A 12. B 20. B5.C 13. C 21. B6.A 14. B 22. C7.B 15. A 23. A8.B 16. D 24. D

25. B