Chemistry

Problem

For the reaction

\text{A}\rightleftharpoons\text{B}

, the standard Gibbs free energy change at

298\,\text{K}

\Delta G^{\circ}=+15.0\;\text{kJ mol}^{-1}

. Assuming this value of

\Delta G^{\circ}

is temperature-independent, calculate the equilibrium constant

K

350\,\text{K}

. (Use

R=8.314\;\text{J mol}^{-1}\,\text{K}^{-1}

.) a)

7.6\times10^{-2}

9.9\times10^{-1}

5.8\times10^{-3}

2.3\times10^{-3}