1 eq for a certain reaction will change if __________ changes.A) pressure B) time C) volume D) temperature E) reactant concentrations 2 2 (g) ↔ N2 O4 (g);2 O4 (g) ↔ 2 NO2 (g)A) Keq of reaction (1) is the reciprocal of Keq of reaction (2). B) Keq of reaction (2) is the reciprocal of Keq of reaction (1) C) Keq of reaction (1) = Keq of reaction (2) D) Answers A and B are both correct E) There is no relationship between the Keq s of these reactions 3 2 (g) → 2 CuO(s)A) Keq = 1/[O2 ]2 B) Keq = [CuO]2 /[Cu]2 C) Keq = [CuO]2 /[Cu]2 [O2 ] D) Keq = [O2 ] E) Keq = 1/[O2 ] 4 2 (g) + O2 (g) ↔ 2 SO3 (g). If, at equilibrium at a certain temperature, [SO2 ] = 1.50 M, [O2 ] = 0.120 M, and [SO3 ] = 1.25 M, what is the value of the equilibrium constant?A) 5.79 B) 6.94 C) 8.68 D) 0.14 E) None of the above 5 5 dissociates according to the reaction: PCl5 (g) ↔ PCl3 (g) + Cl2 (g). One mole of PCl5 was placed in one liter of solution. When equilibrium was established, 0.5 mole of PCl5 remained in the mixture. What is the equilibrium constant for this reaction?A) 0.25 B) 0.5 C) 1.0 D) 2.5 E) None of the above 6 4 . At some temperature, the equilibrium constant for this reaction is 0.30. If the reaction is started with 0.10 mol of SiCl4 in a one-liter flask, how much Cl2 will be present when equilibrium is established?A) 0.18 mol B) 0.090 mol C) 0.030 mol D) 0.30 mol 7 2 (g) + H2 (g) ↔ CO(g) + H2 O(g), for which Kc = 0.64 at 900 K. If the initial CO2 and of H2 are each 0.100 M, what will be the equilibrium concentrations of each species after the reaction reaches equilibrium?A) [CO2 ] = 0.044 M; [H2 ] = 0.044M; [CO] = 0.056 M; [H2 O] = 0.056 M B) [CO2 ] = 0.056 M; [H2 ] = 0.056 M; [CO] = 0.044 M; [H2 O] = 0.044 M C) [CO2 ] = 0.020 M; [H2 ] = 0.020 M; [CO] = 0.080 M; [H2 O] = 0.080 M D) [CO2 ] = 0.080 M; [H2 ] = 0.080 M; [CO] = 0.020 M; [H2 O] = 0.020 M E) None of the above 8 - ↔ ClO3 - + 2 Cl- has an equilibrium constant Kc = 3.2 x 103 . If the components of this reaction are mixed such that their initial concentrations are [Cl- ] = 0.05 M; [ClO3 - ] = 0.32; and [ClO- ] = 0.74, is the mixture at equilibrium, yes or no? If the mixture is not at equilibrium in which direction, left to right or right to left, will reaction occur so that the mixture can reach equilibrium?A) There is not enough information given to answer this question B) Yes, the mixture is at equilibrium now C) No. Left to right D) No. Right to left 9 2 (g) + I2 (g) ↔ 2 HI(g). If the temperature is increased,A) more HI will be produced B) some HI will decompose, forming H2 and I2 C) the magnitude of the equilibrium constant will decrease D) the pressure in the container will increase E) the pressure in the container will decrease 10 2 (g) + CO(g) ↔ NO(g) + CO2 (g). Suppose the volume of the system is decreased at constant temperature, what change will this cause in the system?A) A shift to produce more NO B) A shift to produce more CO C) A shift to produce more NO2 D) No shift will occur 11 A) Chemical equilibrium is a reversible process with no net change in concentrations of the products and reactants. B) Physical equilibrium can not exist between phases. C) A chemical equilibrium with all reactants and products in the same phase is homogeneous. D) none of the above 12 A) catalyst B) pressure C) concentration D) temperature 13 A) Le Chatelier's principle B) Haber process C) Equilibrium constant D) Bosch theory 14 A) True B) False
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