A mixture of 2.0 mol of CO(g) and 2.0 mol of H_2O(g) was allowed to come to equi

Question

A mixture of 2.0 mol of CO(g) and 2.0 mol of H_2O(g) was allowed to come to equilibrium in a 10.0-L flask at a high temperature. If K_c = 4.0, what is the molar concentration of H_2(g) in the equilibrium mixture? The equation for the reaction is this. CO(g) + H_2O(g) CO_2(g) + H_2(g) (A) 0.67 M (B) 0.40 M (C) 0.20 M D) 0.13 M Consider this reaction. 2SO_3(g) 2SO_2(g) + O_2(g) What is the correct K_p expression for this reaction? (A) K_p = P^2_SO_2 P_O_2/P^2_SO_3 (B) K_p = P_SO_2 P_O_2/P_SO_3 (C) K_p = (2 P_SO_3)^2 P_O_2/(2 P_SO_3)^2 (D) K_p = 2P^2_SO_2 P_O_2/2 P^2_SO_3 When a sample of NO_2 is placed in a container, this equilibrium is rapidly established. 2NO_2(g) N_2O_4 (g) If this equilibrium mixture is a darker color at high temperatures or at low pressures, which about the reaction is true? (A) The reaction is exothermic and NO_2 is darker in color than N_2O_4. (B) The reaction is exothermic and N_2O_4 is darker in color than NO_2. (C) The reaction is endothermic and NO_2 is darker in color than N_2O_4. (D) The reaction is endothermic and N_2O_4 is darker in color than NO_2. Consider this reaction. AB_3 (g) A(g) + 3B(g) What is the equilibrium constant expression if the initial concentration of AB_3 is 0.1 M and equilibrium concentration of A is represented by x? Assume the initial concentrations of A are both zero. (A) x - 3x/0.1 - x (B) x - x^3/(0.1 - x)^3 (C) x middot x^3/(0.1 - 3x)^3 (D) x middot (3x)^3/0.1 - x

Explanation / Answer

10. 2SO3(g)<---> 2SO2(g) + O2(g)

Kp is the product of the pressure of each product raised to their stiochiometric coefficients divided by the product of the pressure of reactants raised to their stiochiometric coefficients.

So for this reaction,

Kp = (Pso2)2(Po2)/(Pso3)2

So option A.

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