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)

Question

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) The equilibrium constant,KP,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 Kc? (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.

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

2NOCl(g)
What is the value of K_c? (R = 0.08206 L • atm/K • mol)

Quizplus · Accepted Answer

The equilibrium constant for a reaction in terms of concentrations (Kc) is related to the equilibrium constant in terms of partial pressures (KP) by the equation:

Kc = KP(RT)^(Δn)

Where R is the gas constant, T is the temperature in Kelvin, and Δn is the change in the number of moles of gas between the reactants and products (in this case, Δn = (2+1) - 2 = 1).

Rearranging the equation gives:

KP = Kc / (RT)^Δn

Substituting the given values:

Kc = 6.5 × 10^-4
R = 0.08206 L · atm/K · mol
T = 308 K
Δn = 1

KP = (6.5 × 10^-4) / (0.08206 L · atm/K · mol * 308 K)^1

KP = 1.6 × 10^-12 atm

Therefore, the answer is choice C.

The Equilibrium Constant,KP,has a Value of 6

The Equilibrium Constant,K_P,has a Value of 6