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?

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) 2NOCl(g) What is the value of K_c?

Quizplus · Accepted Answer

The equilibrium constant, Kc, is related to the equilibrium constant, KP, by the equation Kc = KP(RT)Δn, where Δn is the difference between the total number of moles of gaseous products and the total number of moles of gaseous reactants in the balanced chemical equation. 
For the reaction given, Δn = (2+0) - (1+1) = 0. 
Thus, Kc = KP(RT)0 = KP. 
Therefore, the value of Kc is equal to the given value of KP, 1.6 × 10^−2mol/L.

The Equilibrium Constant, Kp, Has a Value of 6

The Equilibrium Constant, K_p, Has a Value of 6