The equilibrium constant, K_P, has a value of 6.5 × 10^-4 at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g) + Cl₂(g) 2NOCl(g) What is the value of K_c? (R = 0.08206 L • atm/K • mol) A) 2.5 × 10^-7 B) 6.5 × 10^-4 C) 1.6 × 10^-2 D) 1.7 E) None of these choices is correct.

Question

Quizplus · Accepted Answer

The equilibrium constant, K, is given by the expression: K = (PNOCl)^2 / (PNO)^2 (PCl2) where P is the partial pressure of each species at equilibrium. Using the given equilibrium constant, we can write: 6.5 × 10-4 = (PNOCl)2 / (PNO)2 (PCl2) Solving for (PNOCl)2 / (PNO)2 gives: (PNOCl)2 / (PNO)2 = 6.5 × 10-4 / PCl2 At equilibrium, the total pressure of the system is Ptotal = PNO + PCl2 + PNOCl. We can express each partial pressure in terms of x, the degree of dissociation of NOCl: PNO = 2(1 - x) PNOCl = x PCl2 = (1 - x) Substituting these expressions into the equation above gives: (x)2 / (2(1 - x))2 = 6.5 × 10-4 / (1 - x) Simplifying and solving for x gives: x = 0.02 Substituting this value of x into the equation for K gives: K = (0.02)2 / (0.96)2 = 1.6 × 10-2 Since K_c = K / (RT)3, where R is the gas constant and T is the temperature in Kelvins, we can calculate K_c using the given value of K and R: K_c = 1.6 × 10-2 / (0.08206 L • atm/K • mol)(308 K)3 ≈ 1.6 × 10-12 Therefore, the best choice is C.

The Equilibrium Constant, KP, Has a Value of 6

The Equilibrium Constant, K_P, Has a Value of 6