The value of log10k for a reaction A⇌B is [Given ΔrH298K0=-54.07KJmol-1;ΔrS0=10JK-1 mol-1 and R=8.314 JK-1mol-1; 2.303×8.314×298=5705]

ΔG0=-RTlnKΔrG0=-2.303RTlog10K But ΔrG0=ΔrH0-TΔrS0=-54.07×103-298×10=-57050 JΔrG0=-2.303×8.314×298log10K-57050=-5705log10K∴log10k=10Concept(s): Gibbs free energy