1. Pure iron metal can be produced by the reduction of iron(III) oxide with hydrogen gas.

(a) Write the expression for the equilibrium constant (Kc) for the reversible reaction

Fe2 O3(s) + 3H2(g) ? 2Fe(s) + 3H2 O(g)              ΔH = 98.7 kJ

b) What will happen to the concentration of each reactant and product at equilibrium if more Fe is added?

c) What will happen to the concentration of each reactant and product at equilibrium if H2O is removed?

(d) What will happen to the concentration of each reactant and product at equilibrium if H2 is added?

(e) What will happen to the concentration of each reactant and product at equilibrium if the pressure on the system is increased by reducing the volume of the reaction vessel?

(f) What will happen to the concentration of each reactant and product at equilibrium if the temperature of the system is increased?

2. Hydrogen is prepared commercially by the reaction of methane and water vapor at elevated temperatures. CH4(g) + H2 O(g) ? 3H2(g) + CO(g)

What is the equilibrium constant for the reaction if a mixture at equilibrium contains gases with the following concentrations: CH4, 0.126 M; H2O, 0.242 M; CO, 0.126 M; H2 1.15 M, at a temperature of 760 °C?