1. The first law of thermodynamics states that __________ is conserved. a.matter b.energy c.entropy d.temperature

2. The first law of thermodynamics states that __________ is conserved. a.matter b.energy c.entropy d.temperature

3. Entropy is a measure of the __________ of a system. a.randomness b.internal energy c.temperature d.polarity

4. Entropy is a measure of the __________ of a system. a.randomness b.internal energy c.temperature d.polarity

5. Since entropy is a state function, the change in entropy is equal to its final value __________ its initial value. a.plus b.minus c.multiplied by d.divided by

6. Since entropy is a state function, the change in entropy is equal to its final value __________ its initial value. a.plus b.minus c.multiplied by d.divided by

7. Entropy decreases when: a.gases are formed from liquids. b.liquids are formed from solids. c.solids are formed from gases. d.the number of gas molecules increases during a chemical reaction.

8. Entropy decreases when: a.gases are formed from liquids. b.liquids are formed from solids. c.solids are formed from gases. d.the number of gas molecules increases during a chemical reaction.

9. The third law of thermodynamics states that the entropy of a pure, perfect crystalline substance at absolute zero (0 K) is: a.infinite. b.increasing. c.decreasing. d.zero.

10. The third law of thermodynamics states that the entropy of a pure, perfect crystalline substance at absolute zero (0 K) is: a.infinite. b.increasing. c.decreasing. d.zero.

11. H = enthalpy. S = entropy. T = Kelvin temperature. The Gibbs free energy, G, is: a. H + TS b. H – TS c. H x TS d. H / TS

12. H = enthalpy. S = entropy. T = Kelvin temperature. The Gibbs free energy, G, is: a. H + TS b. H – TS c. H x TS d. H / TS

13. The value of ∆G, the Gibbs free energy change, for a system at equilibrium is: a.positive. b.negative. c.rapidly fluctuating from positive to negative. d.zero.

14. The value of ∆G, the Gibbs free energy change, for a system at equilibrium is: a.positive. b.negative. c.rapidly fluctuating from positive to negative. d.zero.

15. A reaction will be spontaneous at lower temperatures when the sign of  H and  S is

17. Upon heating, limestone (CaCO 3 ) decomposes to CaO and CO 2. Speculate on the sign of  H and  S for this process. CaCO 3 (s) CaO(s) + CO 2 (g)

18. Upon heating, limestone (CaCO 3 ) decomposes to CaO and CO 2. Speculate on the sign of  H and  S for this process. CaCO 3 (s) CaO(s) + CO 2 (g)