Chapter 13, Problem 44E

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

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

${\text{Fe}}_2{\text{O}}_3\left(s\right)+3{\text{H}}_2\left(g\right)\rightleftharpoons 2\text{Fe}\left(s\right)+3{\text{H}}_2\text{O}\left(g\right)$ $\Delta H=98.7\text{kJ}$

(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?

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