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Back to 13.3 Shifting Equilibria: Le Châtelier’s Principle

13.3 Exercise 10

Avg difficulty 2.5

Methanol can be prepared from carbon monoxide and hydrogen at high temperature and pressure in the presence of a suitable catalyst.

(a) Write the expression for the equilibrium constant (Kc) for the reversible reaction
2H2(g)+CO(g)⇌CH3OH(g)ΔH=−90.2kJ2 \text{H}_{2} \left(g\right) + \text{CO} \left(g\right) \rightleftharpoons \text{CH}_{3} \text{OH} \left(g\right) \Delta H = −90.2 \text{kJ}

(b) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if more H2 is added?

(c) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if CO is removed?

(d) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if CH3OH is added?

(e) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if the temperature of the system is increased?

(f) What will happen to the concentrations of H2, CO, and CH3OH at equilibrium if more catalyst is added?

OpenStax Chemistry 2e, 13.3 Shifting Equilibria: Le Châtelier’s Principle, exercise 10

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Adapted from General Chemistry © 2019 Rice University. Licensed under CC BY 4.0. Sources: Chemistry 2e, Chemistry: Atoms First 2e. Imported at revision 32c7196.