For the reaction given below, 2.00 mol of A and 3.00 mol of B are placed in a 6.00-L container. A(g) + 2B(g) C(g) At equilibrium, the concentration of A is 0.255 mol/L. What is the concentration of B at equilibrium? A) 0.255 mol/L B) 0.343 mol/L C) 0.500 mol?l D) 0.510 mol/L E) none of these A sample of ammonia gas was allowed to come to equilibrium at 400 K. 2NH_3(g) N_2(g0 + 3H_2(g) At equilibrium, it was found that the concentration of H_2 was 0.0420 M, the concentration of N_2 was 0.0140 M, and the concentration of NH_3 was 0.222 M. What is K_q for this equilibrium? (R = 0.0821 L - atm(K - mol)) A) 1.70 times 10^-3 B) 4.28 C) 1.95 times 10^-4 D) 2.85 E) 2.26 times 10^-2 In a first- order reaction, the half-life is 138 minutes. What is the rate constant? A) 0.301 s^-1 B) 8.37 times 10^-5 s^-4 C) 1.21 times 10^-4 s^-1 D) 5.02 times 10^-3 s^-1 E) 5740 s^-1 At 400 K, an equilibrium mixture of H_2, I_2, and HI consists of 0.069 mol H-2, 0,068 mol I_2, and 0.13 mol HI in a 4.5-l flask. What is the value of K_p for the following equilibrium? (R = 0.0821 L middot atem (k middot mol)) 2HI(g) H_2(g) + I_2(g) A) 0.29 B) 8.5 C) 0.037 D) 3.4 E) 27 For the reaction IO_3^-(aq) + 51(aq) + 6H'(aq) rightarrow 3I_2(aq) + 3H_2O(I) the rate of disappearance of I^-(aq) at a particular time and concentration is 2.8 times 10^-3 mol/(L middot s). What is the rate of appearance of I_2(aq)? A) 4.7 times 10^-3 mol (L middot s) B) 1.7 times 10^-3 mol/(L middot) C) 8.4 times 10^-3 mol/(L middot) D) -1.7 times 10^-3 mol/(L middot s) E) 6.0 times 10^-3 mol/(L middot s) Consider the following equilibrium: CO_2(g) + H_2(g) CO(g) + H_2O(g); K_e = 1.6 at 1260 K Suppose 0.029 mol CO_2 and 0.022 mol H_2 are placed in a 3.50-L vessel at 1260 K. What is the equilibrium partial pressure of CO(g)? (R = 0.0821 L middot atm/(K middot)) A) 0.65 atm B) 0.21 atm C) 3.6 atm D) 0.86 atm E) 1.5 atm