The value of log10K for a reaction A⇌B is: (Given, ΔrH°298K = −54.07 kJ mol−1, ΔrS°298K = 10 JK−1 mol−1 and R = 8.314 JK−1 mol−1 ; 2.303 × 8.314 × 298 = 5705)
Using,
ΔG° = ΔH° − TΔS°
= –54.07 × 1000 − 298 × 10
= − 57050 J
also,
ΔG° = –2.303 RT log K
–57050 = 5705 log K
Log K = 10
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