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13.4 Exercise 37

Avg difficulty 2.5

Consider the equilibrium

4NO2(g)+6H2O(g)⇌4NH3(g)+7O2(g)4 \text{NO}_{2} \left(g\right) + 6 \text{H}_{2} \text{O} \left(g\right) \rightleftharpoons 4 \text{NH}_{3} \left(g\right) + 7 \text{O}_{2} \left(g\right)

(a) What is the expression for the equilibrium constant (Kc) of the reaction?

(b) How must the concentration of NH3 change to reach equilibrium if the reaction quotient is less than the equilibrium constant?

(c) If the reaction were at equilibrium, how would an increase in the volume of the reaction vessel affect the pressure of NO2?

(d) If the change in the pressure of NO2 is 28 torr as a mixture of the four gases reaches equilibrium, how much will the pressure of O2 change?

OpenStax Chemistry 2e, 13.4 Equilibrium Calculations, exercise 37

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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.