# Problem: 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 reactionFe2O3(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(f) What will happen to the concentration of each reactant and product at equilibrium if the temperature of the system is increased?

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###### Problem Details

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
Fe2O3(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

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