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, K, is defined as: K = [products]^m/[reactants]^n where m and n are the stoichiometric coefficients of the products and reactants, respectively. In this case, the equilibrium constant (K_p) is given as: K_p = [NOCl]^2/([NO]^2[Cl₂]) To calculate the value of the equilibrium constant in terms of concentrations (K_c), we need to use the equation: K = KPRT^(Δn) where KP is the equilibrium constant in terms of partial pressures, R is the gas constant, T is the temperature in Kelvin, and Δn is the difference in moles of gas products and reactants (moles of products - moles of reactants). In this case, Δn = (2 moles of NOCl) - (2 moles of NO + 1 mole of Cl₂) = 0, since the number of moles of gas on either side of the equation is equal. Thus, the equation becomes: K = KPRT^(0) K = KP K_c = KP To convert from KP to KC, we need to use the equation: KP = KC(RT)^(Δn) Rearranging this equation gives: KC = KP/(RT)^(Δn) Plugging in the values for KP and Δn, we get: KC = K_p/(RT)^(Δn) Plugging in the given values and solving, we get: KC = 6.5 × 10^-14/[(0.0821 L·atm/K·mol)(308 K)]^0 KC = 1.6 × 10^-12 Therefore, the correct answer is C) 1.6 × 10^-12.

The Equilibrium Constant, Kp, Has a Value of 6

The Equilibrium Constant, K_p, Has a Value of 6