The equilibrium constants (expressed in atm) for the chemical reaction N₂(g) + O₂(g) 2NO(g) are K_P = 1.1 × 10^-3 and 3.6 × 10^-3 at 2200 K and 2500 K,respectively.
Which statement is true?

Question

The equilibrium constants (expressed in atm)for the chemical reaction N₂(g)+ O₂(g) 2NO(g)are K_P = 1.1 × 10^-3 and 3.6 × 10^-3 at 2200 K and 2500 K,respectively. Which statement is true?

Quizplus · Accepted Answer

According to Le Chatelier's principle, increasing temperature favors the endothermic reaction. In this case, the forward reaction is endothermic, therefore increasing temperature will shift the equilibrium to the right. This means that at 2500 K, more NO(g) will be produced compared to 2200 K. Therefore, the partial pressure of NO(g)will be higher at 2500 K compared to 2200 K, making option B the correct choice. Options A and E are not necessarily true, and option C is incorrect since K_P and K_c are not directly proportional to RT. Option D is not necessarily true, as the total pressure can vary depending on the initial partial pressures of the reactants and products.

The Equilibrium Constants (Expressed in Atm)for the Chemical Reaction N2(g)

The Equilibrium Constants (Expressed in Atm)for the Chemical Reaction N₂(g)