CHEM 122 CHEMICAL EQUILIBRIUM CHAP 15 ASSIGN
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1 CHEM 122 CHEMICAL EQUILIBRIUM CHAP 15 ASSIGN PLACE THE LETTER REPRESENTING THE BEST ANSWER TO EACH QUESTION ON THE APPROPRIATE LINE ON THE ANSWER SHEET. FOR OTHER QUESTIONS, CLEARLY WRITE THE ANSWER, INCLUDING UNITS WHEN NECESSARY, ON THE ANSWER SHEET. SHOW ALL WORK ON A SEPARATE SHEET OF PAPER. HAND IN ASSIGNMENT, ANSWER SHEET, AND SCRAP WORK. 1. Which of the following statements is FALSE? A) When K >> 1, the forward reaction is favored and essentially goes to completion. B) When K << 1, the reverse reaction is favored and the forward reaction does not proceed to a great extent. C) When K 1, neither the forward or reverse reaction is strongly favored, and about the same amount of reactants and products exist at equilibrium. D) K >> 1 implies that the reaction is very fast at producing products. E) None of the above. 2. Express the equilibrium constant for the following reaction. CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O(g) A) K = B) K = C) K = D) K = E) K = 3. The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant. H2(g) + Br2(g) 2HBr(g) Kc = HBr(g) H2(g) + Br2(g) Kc =? A) B) C) D) E) The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant. 2 SO2(g) + O2(g) 2 SO3(g) Kc = SO3(g) 1/2 O2(g) + SO2(g) Kc =? A) B) 8.5 C) D) E) In a reaction mixture containing only reactants, what is the value of Q? A) -1 B) 1 C) D) 0 E) It cannot be determined without concentrations. 6. In which of the following reactions will Kc = Kp? A) 4 NH 3 (g) + 3 O 2 (g) 2 N 2 (g) + 6 H 2 O(g) B) SO 3 (g) + NO(g) SO 2 (g) + NO 2 (g) C) 2 N 2 (g) + O 2 (g) 2 N 2 O(g) D) 2 SO 2 (g) + O 2 (g) 2 SO 3 (g) E) None of the above reactions have Kc = Kp. 1 P a g e
![Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [P4O10]eq = 2.000 moles, [P4]eq = 3.000 moles, [O2]eq = 4.](/docs-images/81/83018179/images/2-1.jpg "000 M P 4 O 10 (s) P 4 (s) + 5 O 2 (g) A) 20.00 B) 4.000 C) 1.320 D) 1536 E) 1024 10.")
2 7. The reaction below has a Kp value of What is the value of Kc for this reaction at 700 K? 2 SO 3 (g) 2 SO 2 (g) + O 2 (g) A) B) C) D) E) Express the equilibrium constant for the following reaction. Pb(NO 3 ) 2 (aq) + 2 NaI(aq) PbI 2 (s) + 2 NaNO 3 (aq) A) K = B) K = C) K = D) K = E) K = 9. Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [P4O10]eq = moles, [P4]eq = moles, [O2]eq = M P 4 O 10 (s) P 4 (s) + 5 O 2 (g) A) B) C) D) 1536 E) Determine the value of Kp for the following reaction if the equilibrium concentrations are as follows: P(CO)eq = atm, P(O2)eq = atm, P(CO2)eq = atm. 2 CO(g) + O2(g) 2 CO2(g) A) B) C) D) E) Calculate P [NO] eq, if P [NOCl]eq = 0.33 atm, P [Cl2]eq = 0.50 atm, and Kp = NOCl(g) 2 NO(g) + Cl2(g) A) 1.7 atm B) atm C) 0.30 atm D) atm E) atm 12. In a reaction mixture containing reactants and products, each at a concentration of 1M, what is the value of Q? A) -1 B) 1 C) D) 0 E) It cannot be determined without concentrations. 13. Which of the following statements is TRUE? A) If Q < K, it means the reverse reaction will proceed to form more reactants. B) If Q > K, it means the reverse reaction will proceed to form more reactants. C) If Q = K, it means the reaction is not at equilibrium. D) All of the above are true. E) None of the above are true. 2 P a g e
3 14. Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium pressure of CO. CO(g) + 2 H2(g) CH3OH(l) Kp = P(H2)eq = 0.52 atm A) atm B) atm C) atm D) atm E) atm 15. Consider the following reaction: Xe(g) + 2 F2(g) XeF4(g) A reaction mixture initially contains 2.24 atm Xe and 4.27 atm F2. If the equilibrium pressure of Xe is 0.34 atm, find the equilibrium constant (Kp) for the reaction. A) 25 B) 0.12 C) 0.99 D) 8.3 E) Consider the following reaction: CH4(g) + 2 H2S(g) CS2(g) + 4 H2(g) A reaction mixture initially contains 0.50 M CH4 and 0.75 M H2S. If the equilibrium concentration of H2 is 0.44 M, find the equilibrium constant (Kc) for the reaction. A) 0.23 B) C) 2.9 D) 10. E) Consider the following reaction: COCl2(g) CO(g) + Cl2(g) A reaction mixture initially contains 1.6 M COCl2. Determine the equilibrium concentration of CO if Kc for the reaction at this temperature is Calculate this based on the assumption that the answer is negligible compared to 1.6. A) M B) M C) M D) M E) M 18. Consider the following reaction: CuS(s) + O2(g) Cu(s) + SO2(g) A reaction mixture initially contains 2.9 M O2. Determine the equilibrium concentration of O2 if Kc for the reaction at this temperature is 1.5. A) 1.9 M B) 1.7 M C) 2.2 M D) 1.2 M E) 0.59 M 19. Consider the following reaction: 2 H2O(g) + 2 SO2(g) 2 H2S(g) + 3 O2(g) A reaction mixture initially contains 2.8 M H2O and 2.6 M SO2. Determine the equilibrium concentration of H2S if Kc for the reaction at this temperature is A) M B) M C) M D) M E) 0.12 M 20. Consider the following reaction: CO2(g) + C(graphite) 2 CO(g) A reaction mixture initially contains 0.56 atm CO2 and 0.32 atm CO. Determine the equilibrium pressure of CO if Kp for the reaction at this temperature is A) 0.83 atm B) 0.31 atm C) 0.26 atm D) 0.58 atm E) 0.42 atm 3 P a g e
4 21. Consider the following reaction: NO(g) + SO3(g) NO2(g) + SO2(g) A reaction mixture initially contains 0.86 atm NO and 0.86 atm SO3. Determine the equilibrium pressure of NO2 if Kp for the reaction at this temperature is A) 0.78 atm B) atm C) atm D) 0.85 atm E) atm 22. Consider the following reaction at equilibrium. What will happen if Fe 2 O 3 is added to the reaction? 4 FeS 2 (s) + 11 O 2 (g) 2 Fe 2 O 3 (s) + 8 SO 2 (g) A) The equilibrium constant will increase. B) The equilibrium will change in the direction of the reactants. C) The equilibrium will change in the direction of the products. D) No change in equilibrium is observed. E) The equilibrium constant will decrease. 23. Consider the following reaction at equilibrium. What will happen if the pressure increased? 4 FeS 2 (s) + 11 O 2 (g) 2 Fe 2 O 3 (s) + 8 SO 2 (g) A) The equilibrium constant will increase. B) The equilibrium will change in the direction of the reactants. C) The equilibrium will change in the direction of the products. D) No change in equilibrium is observed. E) The equilibrium constant will decrease. 24. The following reaction is exothermic. Which change will shift the equilibrium to the left? 2 SO2(g) + O2(g) 2 SO3(g) A) raising the temperature B) decrease pressure C) increase volume D) all of the above E) none of the above 25. Consider the following reaction at equilibrium. What effect will adding more SO3 have on the system? SO2(g) + NO2(g) SO3(g) + NO(g) A) The reaction will shift in the direction of products. B) The reaction will shift to decrease the pressure. C) No change will occur since SO3 is not included in the equilibrium expression. D) The reaction will shift in the direction of reactants. E) The equilibrium constant will decrease. 26. Consider the following reaction at equilibrium. What effect will removing H2O have on the system? 2 H2S(g) + 3 O2(g) 2 H2O(g) + 2 SO2(g) A) The reaction will shift to the left. B) No change will be observed. C) The equilibrium constant will decrease. D) The equilibrium constant will increase. E) The reaction will shift in the direction of products. 4 P a g e
5 27. Consider the following reaction at equilibrium. What effect will increasing the volume of the reaction mixture have on the system? 2 H2S(g) + 3 O2(g) 2 H2O(g) + 2 SO2(g) A) The reaction will shift to the right in the direction of products. B) No effect will be observed. C) The reaction will shift to the left in the direction of reactants. D) The equilibrium constant will decrease. E) The equilibrium constant will increase. 28. Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system? C3H8(g) + 5 O 2 (g) 3 CO 2 (g) + 4 H 2 O(l) ΔH = kj A) The reaction will shift to the right in the direction of products. B) The reaction will shift to the left in the direction of reactants. C) The equilibrium constant will increase. D) The equilibrium constant will decrease. E) No effect will be observed. 29. Consider the following reaction at equilibrium. What effect will reducing the pressure have on the system? C 3 H 8 (g) + 5 O 2 (g) 3 CO 2 (g) + 4 H 2 O(l) ΔH = kj A) The reaction will shift to the right in the direction of products. B) The reaction will shift to the left in the direction of reactants. C) The equilibrium constant will increase. D) The equilibrium constant will decrease. E) No effect will be observed. 30. The equilibrium constant is equal to 5.00 at 1300 K for the reaction: 2 SO2(g) + O2(g) 2 SO3(g). If initial concentrations are [SO2] = 6.00 M, [O2] = 0.45 M, and [SO3] = 9.00 M, the system is A) at equilibrium. B) not at equilibrium and will remain in an unequilibrated state. C) not at equilibrium and will shift to the left to achieve an equilibrium state. D) not at equilibrium and will shift to the right to achieve an equilibrium state. EXTRA CREDIT 31. The equilibrium constant, Kp, equals 3.40 for the isomerization reaction: cis-2-butene trans-2-butene. If a flask initially contains atm of cis-2-butene and atm of trans-2-butene, what is the equilibrium pressure of each gas? A) P(cis-2-butene) = atm and P(trans-2-butene) = atm B) P(cis-2-butene) = atm and P(trans-2-butene) = atm C) P(cis-2-butene) = atm and P(trans-2-butene) = atm D) P(cis-2-butene) = atm and P(trans-2-butene) = atm 32. Kc is at 25 C for the formation of iron(iii) oxalate complex ion: Fe 3+ (aq) + 3 C 2 O 4 2- (aq) [Fe(C2 O 4 ) 3 ] 3- (aq). If M Fe3+ is initially mixed with 1.00 M oxalate ion, what is the concentration of Fe3+ ion at equilibrium? A) M B) M C) M D) M 5 P a g e
6 33. The reaction below has a Kp value of 41. What is the value of Kc for this reaction at 400 K? N 2 (g) + 3 H 2 (g) 2 NH 3 (g) A) B) C) 26 D) E) At a certain temperature, bromine and nitric oxide react to form nitrosyl bromide: Br 2 (g) + 2 NO (g) 2 NOBr (g). When initial amounts of Br2, NO, and NOBr are mixed, the concentration of NOBr increases. Which statement below is TRUE? A) Kc < Q B) Kc > Q C) Kc = Q D) More information is needed to make a statement about Kc. 35. The equilibrium constant is given for two of the reactions below. Determine the value of the missing equilibrium constant. A(g) + B(g) AB(g) Kc = 0.24 AB(g) + A(g) A2B(g) Kc = A(g) + B(g) A2B(g) Kc =? A) 4.0 B) 0.91 C) 3.6 D) 16 E) NAME DATE ANSWER SHEET CHEM 122 CHAP 15 ASSIGN SPRING P a g e
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