What is the relation between equilibrium constants K_p and K_c for a general gaseous reaction?
Answer and explanation
Correct answer: D. K_p = K_c (R T)^(Delta n)
- Step 1: Using ideal gas law P_i = (n_i / V) R T = C_i R T for partial pressures. Step 2. Substituting into the equilibrium constant expression yields K_p = K_c (R T)^(Delta n), where Delta n is the change in moles of gas. Answer: K_p = K_c (R T)^(Delta n). Why not the others: K_c = K_p (RT)^(Delta n) inverts relation; K_p = K_c / (RT) assumes Delta n = -1; Delta n power sign is positive on right side.
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