1) Calculate the equilibrium constant, Keq, for the following reaction at 25 °C, if [NO]eq = 0.106 M, [O2]eq = 0.122 M and [NO2]eq = 0.129 M. 2 NO (g) + O2 (g) ⇆ 2 NO2 (g)   2) Find the equilibrium constant, Keq, for the following equilibrium. The initial concentrations of AB and A2D are 0.30 M before they are mixed and when equilibrium is reached, the equilibrium concentration of A2D is 0.20 M. 2 AB (g) + C2D (s) ⇆ A2D (g) + 2 CB (s) 3) When 1.00 mol of A and 0.800 mol of B are placed in a 2.00L container and allowed to come to equilibrium, at that time D has a concentration of 0.20M. What is the value of K at equilibrium? 2A (aq) + B (aq) ⇆ C(g) + D(g) 4) What is the equilibrium concentration of Br2 if [HBr] = 0.35 M and [H2] = 0.22M at equilibrium? H2(g) + Br2(g) ⇆ 2HBr(g) K = 62.5  5) For the following hypothetical equilibrium, what is the value of the equilibrium constant if the concentration at equilibrium are as shown? [A] = 4.5 x 10 -5 , [B] = 2.2x 10 -2 , [C]= 9.4 x 10 -3, [D]=1.2 x 10 -2 A(aq) + 2B(aq) ⇆ 2C(aq) + D(aq)  6) What is the equilibrium concentration of C? [A] = 4.5 x 10 -4 ; [B] = 0.25; [D]= 1.4 x 10 -3, A(g) + B(g) ⇆ 2C(g) + D(g) K = 6.0 x 10 -7

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