e5_132_f08 - CHE 132 Final Exam, Fall 2008 Multiple Choice...

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CHE 132 Final Exam, Fall 2008 Multiple Choice On the Scantron form, bubble in the letter of the one choice that best completes the statement or answers the question. No credit will be given for multiple answers. ____ 1. Which of the following represents the most basic solution? A. [OH ] = 1.0 mol L –1 B. [H 3 O + ] = 0.6 10 –14 mol L –1 C. pOH = 2.51 D. [OH ] = 1.0 10 –14 M E. pH = 14.3 ____ 2. Which one of the following is the correct equilibrium constant expression for the reaction given? Zn(s) + CO 2 (g) ZnO(s) + CO(g) A. K c = [Zn] 1 [CO 2 ] 1 [ZnO] [CO] B. K c = [CO 2 ] 1 [ZnO] [CO] C. K c = [Zn] [CO 2 ] [ZnO] 1 [CO] 1 D. K c = [Zn] [CO 2 ] 1 [ZnO] 1 [CO] E. K c = [CO 2 ] 1 [CO] ____ 3. Nitrogen and hydrogen react to form ammonia by the reaction (1/2) N 2 (g) + (3/2) H 2 (g) NH 3 (g) If a mixture of the three gases was in equilibrium, what would be the effect on the amount of NH 3 if the mixture was compressed? A. The amount of ammonia would decrease. B. The amount of ammonia would not change. C. The amount of ammonia would increase. D. To provide an answer we need to know the initial composition of the system. E. To provide an answer we need to know if Δ G ° is negative.
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____ 4. The rate constant of a first order reaction is 2.5 × 10 –5 s –1 . What is the rate of the reaction when the reactant is at a concentration of 2.0 mol L –1 ? A. rate = 1.25 × 10 –5 mol L –1 s B. rate = 0.80 × 10 5 mol –1 L s –1 C. rate = 5.0 × 10 –5 mol L –1 s –1 D. rate = 1.0 × 10 –4 mol 2 L –2 s –1 E. rate = 1.25 × 10 –5 s –1 ____ 5. When, keeping the pressure constant, 229.0 J of energy is supplied as heat to 3.0 mol of argon, the temperature of the sample increases by 2.55 K. Calculate the molar heat capacity of the gas. A. 89.80 J K 1 mol 1 B. 29.93 J K 1 mol 1 C. 0.277 J K 1 mol 1 D. 12.47 J K 1 mol 1 E. To be able to answer we need to know the work done of the system. ____ 6. The equilibrium constants for the following reactions have been measured at 823 K: CoO(s) + H 2 (g) Co(s) + H 2 O(g) K = 67 CoO(s) + CO(g) Co(s) + CO 2 (g) K = 490 From these data, calculate the equilibrium constant for the reaction CO 2 (g) + H 2 (g) CO(g) + H 2 O(g) . A. K = 53.5 B. K = 0.14 C. K = 0.0187 D. K = 423. E. K = 7.31
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____ 7. The rate constant for the reaction C 2 H 4 (g) + H 2 (g) C 2 H 6 (g) has the values 6.98 × 10 –9 L mol –1 s –1 at 500.0 K and 4.16 × 10 –6 L mol –1 s –1 at 600.0 K. What is the value of the ratio ( E a / R ), where E a is the activation energy and R is the gas constant? A. 6.390 kJ mol –1 B. 8923 °C C. 53127 J K –1 mol –1 D. 19171 K E. 8326 L mol –1 s –1 ____ 8. It required 17.6 mL of 0.014 mol L –1 aqueous KOH solution to titrate a 25.0 mL sample of HCl to the equivalence point. Calculate the molarity of the HCl solution. A. 0.0099 mol L
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This note was uploaded on 03/06/2012 for the course CHE 132 taught by Professor Hanson during the Fall '08 term at SUNY Stony Brook.

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e5_132_f08 - CHE 132 Final Exam, Fall 2008 Multiple Choice...

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