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Back to 13.3 Shifting Equilibria: Le Châtelier’s Principle

13.3 Exercise 12

Avg difficulty 2.5

Water gas, a mixture of H2 and CO, is an important industrial fuel produced by the reaction of steam with red hot coke, essentially pure carbon.

(a) Write the expression for the equilibrium constant for the reversible reaction
C(s)+H2O(g)⇌CO(g)+H2(g)ΔH=131.30kJ\text{C} \left(s\right) + \text{H}_{2} \text{O} \left(g\right) \rightleftharpoons \text{CO} \left(g\right) + \text{H}_{2} \left(g\right) \Delta H = 131.30 \text{kJ}

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

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

OpenStax Chemistry 2e, 13.3 Shifting Equilibria: Le Châtelier’s Principle, exercise 12

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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.