Ammonia Is Prepared Industrially by the Following Reaction: N₂(g) $\Delta$ H° = -922 KJ and K (At 25°C) = 4

Ammonia is prepared industrially by the following reaction: N₂(g) + 3H₂(g) 2NH₃(g)
For the reaction, $\Delta$ H° = -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 statements is true?

A) Product formation (at equilibrium) is not favored as the temperature is raised.
B) K for the reaction will be larger at 500°C than at 25°C.
C) The reaction of N₂ with H₂ to form ammonia is endothermic.
D) At equilibrium, more NH₃ is present at 500°C than at 25°C.
E) None of these is true.