Ammonia is prepared industrially by the following 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 statements is true?

Question

Ammonia is prepared industrially by the following reaction:
N₂(g) + 3H₂(g)

Ammonia is prepared industrially by the following reaction: N<sub>2</sub>(g) + 3H<sub>2</sub>(g) 2NH<sub>3</sub>(g) For the reaction, ΔH° = -92.2 kJ and K (at 25°C) = 4.0 × 10<sup>8</sup>. 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 N<sub>2</sub> with H<sub>2</sub> to form ammonia is endothermic. D) At equilibrium, more NH<sub>3</sub> is present at 500°C than at 25°C. E) None of these is true.

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 statements is true?

Quizplus · Accepted Answer

The Answer of Ammonia is prepared industrially by the following 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 statements is true?

Ammonia Is Prepared Industrially by the Following Reaction