# Final_Exam_2006_with_Answers - Monday December 18th 2006...

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Monday, December 18 th , 2006 Question 1. For the reaction, CO (g) + H 2 O (g) CO 2(g) + H 2(g) K c = 4.06 at 500 °C. If 0.10 mol of CO (g) and 0.10 mol of H 2 O (g) are placed in a 1.0 L reaction vessel at 500 °C, what is the molar concentration (in mol·L –1 ) of CO 2 once the system has reached equilibrium? A. 0.015 B. 0.033 C. 0.067 D. 1.01 E. 2.03 Question 2. At 390 K, the K c for the equilibrium below is 1.83 × 10 –3 mol·L –1 . PCl 5(g) PCl 3(g) + Cl 2(g) Assume a quantity of PCl 5(g) is placed in a 10 L vessel and the system is allowed to reach equilibrium at a constant temperature of 390 K. Identify the single correct or incorrect statement from those given below. A. If the number of moles of PCl 5(g) in the vessel is 1 when the reaction is at equilibrium then the number of moles of both Cl 2(g) and PCl 3(g) are 0.043. B. If some of the equilibrium mixture is removed, a new equilibrium mixture will eventually form and the mole fractions of the three components will be the same as for the original equilibrium mixture. C. Higher mole fractions of Cl 2 and PCl 3 will result if the volume is halved. D. If the volume of the vessel is doubled, the value of Q immediately after the change in volume will be 9.15 × 10 –4 mol·L –1 . E. Based on the original quantity of PCl 5 , higher mole fractions of Cl 2 and PCl 3 will be obtained if a catalyst is added to the system. Question 3. Consider the following equilibrium reaction: 3 NO (g) N 2 O (g) + NO 2(g) The equilibrium constant, K p , is measured to be: 1.8 × 10 18 atm –1 at 25 °C 2.0 × 10 11 atm –1 at 127 °C Estimate K p (in atm –1 ) at 254 °C. D.1.6 × 10 11 E. 1.9 × 10 18

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