In the Haber process for making ammonia, an increase in pressure favors

Explanation

The correct answer is that an increase in pressure favors the forward reaction in the Haber process. This is because the forward reaction results in fewer gas molecules: N2 + 3H2 ↔ 2NH3. With an increase in pressure, the system will adjust to minimize this change by favoring the production of fewer gas molecules, hence the forward reaction is favored. Option B is incorrect as the reverse reaction would increase the number of gas molecules, opposing the pressure increase. Option C is incorrect because the pressure change does affect equilibrium, and therefore one reaction is favored. Option D is incorrect since both reactions cannot be favored at the same time with respect to pressure changes.