Question

At 400 K, an equilibrium mixture of H_2, I_2, and HI consists of 0.068 mol H_2, 0.075 mol I_2, and 0.13 mol HI in a1.00-L flask. What is the value of K_p, for the flowing equilibrium? (R = 0.0821 L middot atm (K - mol)) 2HI_(g) Rightwardsharpoonoverleftwardsharpoon H_2 (g) + I_2 (g) A) 0.039 B) 3.4 C) 26 D) 0.29 E) 8.2 If K = 0.150 for A_2 + 2B Rightwardsharpoonoverleftwardsharpoon 2AB, what is the value of K for the reaction 4AB Rightwardsharpoonoverleftwardsharpoon 2A_2 + 4B? A) 3.33 B) 0.300 c) 44.4 D) -0.150 E) 0.150 For which of the following equilibria does K_c = K_p ? A) CaO () + CO_2 (g) Rightwardsharpoonoverleftwardsharpoon CaCO_2 () B) N_2 (g) + 3H_2 (g) Rightwardsharpoonoverleftwardsharpoon 2NH_2(g) C) CO(g) + 3H_2 (g) Rightwardsharpoonoverleftwardsharpoon CH_1 (g) + H_2 O (g) D) CO(g) + H_2 O (g) Rightwardsharpoonoverleftwardsharpoon CO_2 (g) + H_2(g) E) HBr(g) Rightwardsharpoonoverleftwardsharpoon 1/2 H_2 (g) + 1/2 Br_2 (I) A solution has a hydroxide-ion concentration of 0.0010 M. What is the pOH of the solution? A) 11.0 B) 6.9 C) 7.1 D) 3.0 E) 7.0 The reaction quotient for a system is 7.2 times 10^2. If the equilibrium constant for the system is 36, what will happen as equilibrium is approached? A) There will be a net gain in both product and reactant. B) There will be a net gain in product. C) There will be no net gain in product. D) The equilibrium constant will decrease until it equals the reaction quotient. E) There will be a net gain in reactant.

Answer 1

Find the An, Change in moles of gas = no, of moles of gas in products-no, of moles of gas in reactants So Kp-Ke(RT Kp Kc(RT) - Ke Hence HI (0.068 x 0.075) Кр AC- (013) 0.300.29 is the answer