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. Since the forward reaction in this case is endothermic (it absorbs heat), increasing the temperature will favor the formation of products. Therefore, at the higher temperature of 2,500 K, the equilibrium constant is greater, indicating that there is more NO(g) present in the system, which means its partial pressure is higher at 2,500 K than at 2,200 K.

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