1 A) the concentrations of reactants is equal to the concentrations of products B) the limiting reagent has been completely depleted C) the rate of the forward reaction equals the rate of the reverse reaction D) A and B. 2 2 (g) ↔ 2 NO(g) + O2 (g)A) Keq = [O2 ]2 [NO]/[NO2 ]2 B) Keq = [O2 ][NO]2 /[NO2 ]2 C) Keq = [NO2 ]2 /[NO]2 [O2 ] D) Keq = [NO2 ]2 /[NO][O2 ]2 E) None of the above 3 3 (g) → N2 (g) + 3 H2 (g) is 3 x 10-3 at some temperature. What is Keq for the reaction 0.5 N2 (g) + 1.5 H2 (g) ↔ NH3 (g) at the same temperature?A) 0.003 B) 0.05 C) 18 D) 20 4 3 ): N2 (g) + 3 H2 (g) ↔ 2 NH3 (g) for which Kc at 300 o C is 9.5. Calculate Kp for this reaction at 300 o C.A) Kp = 4.3 x 10-3 B) Kp = 9.5 C) Kp = 2.1 x 104 D) Kp = 1.6 x 10-2 5 2 (g) + I2 (g) ↔ 2 HI(g), Kc = 12.3 at some temperature T. If [H2 ] = [I2 ] = [HI] = 3.21 x 10-3 M at that temperature, which one of the following statements is true?A) The concentration of HI will rise as the system approaches equilibrium B) The system is at equilibrium, so the concentrations will not change C) The concentrations of H2 and I2 will increase as the system approaches equilibrium D) The concentrations of H2 and HI will decrease as the system approaches equilibrium E) Not enough information is given to answer the question 6 c for the reaction 2 NH3 (g) ↔ N2 (g) + 3 H2 (g) is 3 x 10-3 at some temperature. A 1.0 L mixture containing 1.0 mol of NH3 , 0.50 mol of N2 , and 0.15 mol of H2 is prepared at this temperature When equilibrium is reached,A) there will be more N2 and H2 present B) there will be more NH3 present C) there will be less N2 but more H2 present. D) there will be less NH3 and less N2 present E) No shift will occur 7 5 ↔ PCl3 + Cl2 is 1.0, how many moles of PCl5 must be placed into one liter of solution in order to obtain 0.50 mol of PCl3 when the system reaches equilibrium?A) 0.25 B) 0.50 C) 0.75 D) 1.00 8 3 Cl + OH- ↔ CH3 OH + Cl- is started with 0.1 mol of CH3 Cl and 0.2 mol of OH- , 0.03 mol of CH3 OH is present when the system reaches equilibrium. Calculate the equilibrium constant for the reaction.A) 0.18 B) 0.08 C) 0.0009 D) 0.30 9 c for the reaction PCl5 (g) ↔ PCl3 (g) + Cl2 (g) is 0.020. If 0.10 mol of PCl5 and 0.20 mol of PCl3 are added to a 1-L flask, what will be the Cl2 concentration when equilibrium is reached?A) 0.020 M B) 8.7 x 10-3 M C) 0.0052 M D) 0.12 M 10 2 (g) + I2 (g) ↔ 2 HI(g) for which, at some temperature, Kc = 4.0. When the reaction is started with equimolar quantities of H2 and I2 and equilibrium is reached, 0.20 mol of HI is present. How much H2 was used to start the reaction?A) 0.10 mol B) 0.23 mol C) 0.20 mol D) 4.0 mol
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