Take R = 8.314 J mol^-1 K^-1. For a reaction, K = 0.25 at 350 K and Delta H deg = +40.0 kJ mol^-1 (constant). Calculate K at 400 K (two decimals).

JEE Main levelNumerical answerDifficulty 2 of 3ce139

Take $R = 8.314 J mo l^{- 1} K^{- 1}$ . For a reaction, $K = 0.25$ at $350 K$ and $Δ H^{\circ} = + 40.0 kJ mo l^{- 1}$ (constant). Calculate $K$ at $400 K$ (two decimals).

Numerical answer type, tolerance 0.02.

ln (K_{2} / K_{1}) = \frac{40000}{8.314} (\frac{1}{350} - \frac{1}{400}) = 1.7183

, so

K_{2} / K_{1} = 5.575

and

K_{2} = 0.25 \times 5.575 = 1.3937

, i.e. 1.39.