Exam 1 Practice Test Problems with Key

# Given the following reaction at equilibrium if k c

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20) Given the following reaction at equilibrium, if K c 6.44 x 10 5 at 230.0 °C, K p = __________. 2 2 2NO (g) O (g) 2NO (g) A) 3.67 x 10 2 B) 1.56 x 10 4 C) 6.44 x 10 5 D) 2.66 x 10 6 E) 2.67 x 10 7 21) The equilibrium constant for reaction 1 is K. The equilibrium constant for reaction 2 is __________. (1) 2 2 3 SO (g) (1/ 2) O (g) SO (g) (2) 3 2 2 2SO (g) 2SO (g) O (g) 22) Consider the following equilibrium. 2 2 3 2 SO (g) O (g) 2 SO (g) The equilibrium cannot be established when __________ is/are placed in a 1.0-L container. A) 0.25 mol SO 2 (g) and 0.25 mol O 2 (g) B) 0.75 mol SO 2 (g) C) 0.25 mol of SO 2 (g) and 0.25 mol of SO 3 (g) D) 0.50 mol O 2 (g) and 0.50 mol SO 3 (g) E) 1.0 mol SO 3 (g)

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23) Which of the following expressions is the correct equilibrium-constant expression for the reaction below? 4 2 3 2 (NH ) Se (s) 2NH (g) H Se (g) A) [NH 3 ][H 2 Se] / (NH 4 ) 2 Se B) (NH 4 ) 2 Se / [NH 3 ] 2 [H 2 Se] C) 1/[(NH 4 ) 2 Se] D) [NH 3 ] 2 [H 2 Se] E) [NH 3 ] 2 [H 2 Se] / [(NH 4 ) 2 Se] 24) Consider the following chemical reaction: 2 2 H (g) I (g) 2 HI (g) At equilibrium in a particular experiment, the concentrations of H 2 , I 2 , and HI were 0.15M 0.033M and 0.55M respectively. The value of K eq for this reaction is __________. 25) Dinitrogen tetroxide partially decomposes according to the following equilibrium: N 2 O 4 (g) 2NO 2 (g) A 1.000-L flask is charged with 3.00 10 2 mol of N 2 O 4 . At equilibrium, 2.36 10 2 mol of N 2 O 4 remains. K eq for this reaction is __________.
26) At 200 °C, the equilibrium constant (K p ) for the reaction below is 2.40 10 3 . 2 2 2NO (g) N (g) O (g) A closed vessel is charged with 36.1 atm of NO. At equilibrium, the partial pressure of O 2 is __________ atm. A) 294 B) 35.7 C) 17.9 D) 6.00 E) 1.50 10 2 27) Which of the following statements is true? A) Q does not change with temperature. B) K eq does not change with temperature, whereas Q is temperature dependent. C) K does not depend on the concentrations or partial pressures of reaction components. D) Q does not depend on the concentrations or partial pressures of reaction components. E) Q is the same as K eq when a reaction is at equilibrium. 28) Of the following equilibria, only __________ will shift to the left in response to a decrease in volume. A) 2 2 H (g) Cl (g) 2 HCl (g) B) 3 2 2 2 SO (g) 2 SO (g) O (g) C) 2 2 3 N (g) 3H (g) 2 NH (g) D) 2 2 3 4 Fe (s) 3O (g) 2Fe O (s) E) 2 2 2HI (g) H (g) I (g) 29) Consider the following reaction at equilibrium: 3 2 2 2NH (g) N (g) 3H (g) ΔH° = +92.4 kJ According to Le Chatelier's principle, which of the following would not be an effect of adding N 2 (g) to the above system at equilibrium? A) an increase in the concentration of NH 3 (g) B) a decrease in the concentration of H 2 (g) C) no change in the equilibrium constant D) a higher partial pressure of N 2 at the new equilibrium position E) absorption of heat

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30) Consider the following reaction at equilibrium.
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