Consider the endothermic reaction: N₂(g) + O₂(g) → 2 NO(g), ΔH° = 192.5 kJ/mol At 2000 K the equilibrium constant is 5.0 × 10^-4. At 2500 K the value of the equilibrium constant: A) is greater than 5.0 × 10^-4 B) depends on the concentration of oxygen C) is 10.0 × 10^-4 D) is 5.0 × 10^-4 E) is less than 5.0 × 10^-4

Question

Quizplus · Accepted Answer

At higher temperatures, the equilibrium constant for endothermic reactions increases because the reaction shifts in the direction of the products, which increases the concentration of products. Therefore, the equilibrium constant at 2500 K will be greater than 5.0 × 10^-4.

Consider the Endothermic Reaction: N2(g) + O2(g) → 2 NO(g)

Consider the Endothermic Reaction: N₂(g) + O₂(g) → 2 NO(g)