In the equilibrium N2O4(g) 2NO2(g) at 400 K, the partial pressures are p_NO2 = 0.50 atm and p_N2O4 = 0.40 atm. Using R = 0.0821 L atm mol^-1 K^-1, calculate K_c in mol L^-1, correct to three decimal places.

JEE Main levelNumerical answerDifficulty 2 of 3ce072

In the equilibrium $N X_{2} O X_{4} (g) 2 NO X_{2} (g)$ at 400 K, the partial pressures are $p_{NO X_{2}} = 0.50$ atm and $p_{N X_{2} O X_{4}} = 0.40$ atm. Using $R = 0.0821 L atm mo l^{- 1} K^{- 1}$ , calculate $K_{c}$ in $mol L^{- 1}$ , correct to three decimal places.

Numerical answer type, answer in mol/L, tolerance 0.001.

K_{p} = (0.50)^{2} /0.40 = 0.625

atm. With

Δ n = + 1

K_{c} = K_{p} / RT = 0.625/ (0.0821 \times 400) = 0.0190 mol L^{- 1}