Ammonia is prepared industrially by the reaction: N2(g) + 3H2(g) 2NH3(g) for the reaction: H = 92.2 kJ and K (at 25C) = 4.0

Ammonia is prepared industrially by the reaction: N2(g) + 3H2(g) 2NH3(g) for the reaction: ΔH° = –92.2 kJ and K (at 25°C) = 4.0 × 108. When the temperature of the reaction is increased to 500°C, which of the following is true?

a. At equilibrium, more NH3 is present at 500°C than at 25°C.

b. The reaction of N2 with H2 to form ammonia is endothermic.

c. K for the reaction will be larger at 500°C than at 25°C.

d. Product formation (at equilibrium) is not favored as the temperature is raised.

e. None of these choices is true.