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Question:

Which of the following statement is correct for a reversible process in a state of equilibrium?

ΔGo=𕒶.303RTlogK

ΔGo=2.303RTlogK

ΔG=𕒶.303RTlogK

ΔG=2.303RTlogK

Solution:

The relationship between the Gibbs free energy change ΔG, the standard Gibbs free energy change ΔGo and the equilibrium constant K is given by:

ΔG = ΔGo + RTlnK

At equilibrium, ΔG = 0. Therefore, the equation becomes:

0 = ΔGo + RTlnK

ΔGo = -RTlnK

Since lnK = 2.303logK, we can rewrite the equation as:

ΔGo = -2.303RTlogK

Therefore, the correct option is ΔGo = -2.303RTlogK. Note that the provided options contain seemingly invalid Unicode characters (𕒶) which likely represent a minus sign. The correct option is missing from the list.