Question

1:Consider the following equilibrium process at 686°C: CO2(g) + H2(g) ⇌ CO(g) + H2O(g) The equilibrium concentrations of the reacting species are [CO] = 0.0570 M, [H2] = 0.0420 M, [CO2] = 0.0860 M, and [H2O] = 0.0430 M. (a) Calculate Kc for the reaction at 686°C. (b)If we add CO2 to increase its concentration to 0.440 mol / L, what will the concentrations of all the gases be when equilibrium is reestablished? (c) CO2: H2: CO: H2O:

2:The following reactions have the indicated equilibrium constants at a particular temperature: N2(g) + O2(g) ⇌ 2NO(g) Kc = 8.7 × 10−25 2NO(g) + O2(g) ⇌ 2NO2(g) Kc = 6.4 × 109 Determine the value of the equilibrium constant for the following equation at the same temperature: 2NO(g) ⇌ N2(g) + O2(g) 2: Be sure to answer all parts. The equilibrium constant Kc for the reaction H2(g) + CO2(g) ⇌ H2O(g) + CO(g) is 4.2 at 1650°C. Initially 0.81 mol H2 and 0.81 mol CO2 are injected into a 5.4−L flask. Calculate the concentration of each species at equilibrium. Equilibrium concentration of H2: Equilibrium concentration of CO2: Equilibrium concentration of H2O: Equilibrium concentration of CO:

3: The following reactions have the indicated equilibrium constants at a particular temperature: N2(g) + O2(g) ⇌ 2NO(g)Kc = 2.4 × 10−25 2NO(g) + O2(g) ⇌ 2NO2(g)Kc = 6.4 × 109 Determine the value of the equilibrium constant for the following equation at the same temperature: 1/2 N2(g) + 1/2 O2(g) ⇌ NO(g)

Answer 1