Question

One way of preparing H2 (g) is given by the reaction of Zn (s) with HCl (aq).

Zn (s) + 2HCl (aq) <=> H2 (g) +ZnCl2 (aq).

The reaction is exothermic and the equilibrium constant is 3.8E5 (3.8 X 10^5) at room temperature (298K). Assuming that the reaction is at equilibrium what are the effects of the following changes on the equilibrium concentration of H2 (g). Explain based on the reaction quotient compared to the equilibrium constant at the point the change is made.

a) Increasing the concentration of HCl (aq) from 0.1 M to 0.2 M.

b) Adding 0.01 M NaOH to the reaction at equilibrium

c) Heating the equilibrium mixture to 450K. Will this equilibrium constant change?

Answer 1