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Exam Review Chapter 18-Equilibrium Key concepts: Collisions theory Factors affecting reaction rates (Incl. affect of catalysts, activation energy) Dynamic equilibrium LeChatelier’s Principle Keq 1. What effect does increasing the concentration have on rates of reactions? a. Increases the number of collisions b. Increases the energy with which molecules collide c. Both a and b d. None of the above 2. Which of the following is not true about the effect of a catalyst a. Permit reactions to proceed along a lower energy path b. Are not used up in the reaction c. Must be combined with increased temperature d. Inhibitors interfere with the effects of a catalyst 3. When 0.1M HCl is added to the following system at equilibrium: AgCl(s) ↔Ag+(aq)+ Cl-(aq) the point of equilibrium will shift to the a. right and the concentration of Ag+(aq) will decrease. b. right and the concentration of Ag+(aq) will increase. c. left and the concentration of Ag+(aq) will decrease. d. left and the concentration of Ag+(aq) will increase. 4. What is the expression for Keq for this reaction? 5. In an equilibrium reaction with a Keq of 1 x108 a. reactants are favored. c. products are favored. b. the reaction is nonspontaneous. d. the reaction is exothermic. 6. What is the effect of adding more CO2 to the following equilibrium reaction? CO2 + H2O↔ H2CO3 a. More H2CO3 is produced. b. More H2O is produced. c. The equilibrium d. No Change 7. Two opposing reactions (A + B ↔C + D) occurring simultaneously at the same rate is an example of: a. reversibility. c. neither a nor b b. chemical equilibrium. d. both a and b 8. According to collision theory, in order for a chemical reaction to occur, the reactant atoms must: a. make contact with each other. b. have a minimum level of kinetic energy. c. form an activated complex. d. all of the above 9. In general, increasing temperature causes the rate of most chemical reactions to: a. increase. c. remain the same. b. decrease. d. vary unpredictably. 10. Which of the following is true concerning the impact of increasing temperature on reaction rates? a. The number of collisions between reactant atoms is increased. b. The energy of each reactant atom is increased. c. The percentage of collisions with sufficient energy to cross the activation energy barrier is increased. d. all of the above 11. Given the following system at equilibrium: N2(g) +3H2(g) ↔2NH3(g) what would be the effect of removing NH3(g) as it is formed? a. The equilibrium would shift to the left. b. More N2(g) would be produced. c. More H2(g) would be produced. d. The equilibrium would shift to the right 12. Given the following system at equilibrium: H2O(l) +heat ↔H2O(g) how would a decrease in temperature affect the system? a. The equilibrium would shift to the right. b. More H2O(l) would be produced. c. More H2O(g) would be produced. d. The levels of reactants and products would remain the same. 13. Which of the following would increase the yield of CO(g) in the following equilibrium system? C(s) +H2O(g) + heat ↔CO(g) + H2(g) a. decreasing temperature c. adding H2(g) b. increasing pressure d. adding H2O(g) 14. What is the expression for Keq for the following reaction? 15. Calculate the value of Keq for this reaction at equilibrium. 2NOCl(g) ↔2NO(g) + Cl2(g) An analysis of the equilibrium mixture in a 1-L flask gives the following results: NOCl, 0.30 mol; NO, 1.2 mol; Cl2, 0.60 mol. 16. Carbon monoxide and hydrogen are combined in the commercial preparation of methyl alcohol. At a certain set of conditions, the equilibrium mixture contains 0.020 mol/L of CO, 0.60 mol/L of H2, and the equilibrium constant is 2.2 x102. What is the concentration of CH3OH in the equilibrium mixture? 17. Predict the changes in the equilibrium position for this reaction when the following changes are made: 2A(g) + B(g) ↔4C(g) + heat a. decrease the concentration of C b. add more heat c. increase the concentration of A d. increase the pressure In each case, state whether the change causes a shift that favors the formation of reactants or of products. 22. A 5.0 L vessel contained 6.0 mol of SO2, 2.5 mol of NO2 and 1.0 mol of SO3. At equilibrium the vessel was found to contain 3.0 mol of SO3. Calculate Keq. SO2 (g) + NO2 (g) ↔ SO2 SO3 (g) + NO (g) NO2 SO3 NO I C E 23. A 10.0 L bulb is filled with 4.0 mol of SO2, 2.2 mol of O2 and 5.6 mol of SO3. After equilibrium of the formation reaction, there was 2.6 mol of SO2. Calculate Keq. 2SO2 (g) + O2 (g) ↔ SO2 I C E 2SO3 (g) O2 SO3