The reaction below has a K_c value of 61 M^-2. What is the value of K_p for this reaction at 500 K? N₂(g) + 3H₂(g) ⇌ 2NH₃(g)

Question

Quizplus · Accepted Answer

The K_p value can be calculated using the equation ΔG° = -RTln(K), where R is the gas constant and T is the temperature in Kelvin. We can assume standard state conditions for the reactants and products, so ΔG° = -RTln(K_c). Plugging in the given values, we get: -ΔG°/RT = ln(K_c) -(61 M^-2)/(8.314 J/K·mol·500 K) = ln(K_c) K_c = e^(-(61 M^-2)/(8.314 J/K·mol·500 K)) = 3.6 × 10^-2 bar^-2. The answer is therefore D.

The Reaction Below Has a Kc Value of 61 M-2

The Reaction Below Has a K_c Value of 61 M^-2