is gas C. solid 3. Which of the following is a A. ripening of fruits B. liquid nonspontaneous process? C. coffee getting colder B. a ball rolling upwards D. a drop of ink dispersing in water 4. What happens to entropy when solid carbon dioxide (dry ice) sublimes? A. It decreases B. it increases C. It stays the same D. cannot be determined 5. What is the value for standard temperature and pressure or STP? A. 25°C and 10 atm B. 25°C and 1 atm C. 100°C and 1 atm D. 32°C and 10 atm 6. Who is the proponent of the Gibbs free energy? A. William Friedrich B. Guglielmo Marconi C. William Gibbs D. Janno Gibbs 7. When AG < 0, the reaction is A. spontaneous in the forward direction C. nonspontaneous in the forward direction B. spontaneous in the backward direction D. at equilibrium. 8. Calculate AS for the following reaction: H2(g) + 12 (s)-> 2H1 (g) if the entropy values for each substance is as follows: H2(g) = 130.6, 12 (s) = 116.7 and Hl (g) = 206.3 A. AS = +165.3 J/K B. AS = -165.3 J/K C. AS = -41 J/K D. AS = +453.6 J/K 9. What value of Gibbs free energy can we safely predict that the reaction is spontaneous at all temperatures? A. a negative value C. a positive value at a low temperature B. a positive value D. a positive value at a high temperature 10. What will be the value of the entropy change of the system B. negative in the reaction: 6CO₂(g) + 6H₂O(g) → C6H12O6(g) + 602(g) ? C. no change D. cannot be determined A. positive 11. Ozone (03) in the atmosphere can react with nitric oxide (NO): Os(g) + NO(g) -> NO2(g) + O2(g) Calculate the G for this reaction at 25°C. (AH = -199 kJ/mol, AS = -4.1 J/K mol) A. -198 kJ/mol B. +198 kJ/mol C.-301.5 kJ/mol D. +301.5 kJ/mol 12. Which of the following is true for a chemical reaction at equilibrium? A. only the forward reaction stops C. both the forward and reverse reactions stop D. the rates of the forward and reverse reactions are equal B. only the reverse reaction stops 13. If the reaction quotient Q has a smaller value than the related equilibrium constant, K, the reaction is: A. the reaction is at equilibrium. B. the reaction is not at equilibrium, and will make more products at the expense of reactants. C. the reaction is not at equilibrium, and will make more reactants at the expense of products. D. the value of K will decrease until it is equal to Q. 3CO2(g) + 4H₂O(g) 14. Write the correct Kc expression for the following reaction: C3Ha (g) +502(g) [C3H8][02]5 [H2014 [CO2]3 A. [H2014 [CO2] 3 [C3H8][02] 5 B. [H20] [CO2] [C3H8][02] C. [C3H8)[02] D. [H20] [CO2] 15. What happens to the total pressure when the volume of the container is increased? A. decreases B. increases C. becomes zero D. remains constant 16. What do you call a chemical reaction that produces heat? A. endothermic B. exothermic C. equilibrium D. none of the choices 17. Where does the equilibrium lie when K has a very large value? A. left B. right C. center D. none of the choice 18. Where will the equilibrium shift when we increase the concentration of a substance in a reaction? A. away from substance B. towards the substance C. no shift D. all directions 19. What does Le Chatelier's principle state about chemical equilibrium? A. If a stress is applied to a system in equilibrium, then the systems adjust in order to increase the cause of the stress applied. B. If a stress is applied to a system in equilibrium, then the systems adjust in order to increase the effect of the stress applied. C. If a stress is applied to a system in equilibrium, then the systems adjust in order to reduce the cause of the stress applied. D. If a stress is applied to a system in equilibrium, then the systems adjust in order to reduce the effect of the stress applied.