The equilibrium constants for the chemical reaction N₂(g)+ O₂(g) 2NO(g)are K_P = 1.1 * 10^-3 and 3.6 * 10^-3 at 2,200 K and 2,500 K, respectively. Which one of these statements is true?

Question

Quizplus · Accepted Answer

According to Le Chatelier's principle, an increase in temperature favors an endothermic reaction, so the equilibrium would shift towards NO(g), which is an endothermic reaction. As the equilibrium constant for the forward reaction increases with increasing temperature, it means that the forward reaction is favored at higher temperatures. Therefore, the partial pressure of NO(g) would be higher at 2,500 K than at 2,200 K, which is indicated by choice B. None of the other options are necessarily true based on the given information.

The Equilibrium Constants for the Chemical Reaction N2(g)+ O2(g) Δ\DeltaΔ Hº < 0 B)The Partial Pressure of NO(g)is Less at 2,200 K

The Equilibrium Constants for the Chemical Reaction N₂(g)+ O₂(g) $\Delta$ Hº < 0
B)The Partial Pressure of NO(g)is Less at 2,200 K