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As per your syllabus, eqn 5.23, the relation between ΔG° and equilibrium constant K is which?
AΔG° = RT K
BΔG° = K/RT
CΔG° = +RT ln K
DΔG° = −RT ln K = −2.303 RT log K
Answer & Solution
Correct answer: D. ΔG° = −RT ln K = −2.303 RT log K
As per your syllabus, eqn 5.23, ΔG° = −RT ln K. Large negative ΔG°
→ K ≫ 1 (favours products). Positive ΔG° → K ≪ 1.
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