Take R = 8.314 J mol^-1 K^-1. A reaction has K = 2.0 x 10^4 at 300 K. The standard Gibbs energy change at 300 K is

JEE Main levelSingle correct optionDifficulty 2 of 3ce133

Take $R = 8.314 J mo l^{- 1} K^{- 1}$ . A reaction has $K = 2.0 \times 1 0^{4}$ at $300 K$ . The standard Gibbs energy change at $300 K$ is

Δ G^{\circ} = - RT ln K = - (8.314) (300) ln (2.0 \times 1 0^{4}) /1000 = - (2494.2) (9.903) /1000 = - 24.7 kJ mo l^{- 1}

. Using

lo g_{10}

gives -10.7 and using

T = 27

instead of

300 K

gives -2.22, both wrong.