The correct relationship between free energy change in a reaction and the corresponding equilibrium constant Kc is:

Δ G = R T l n K c

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- Δ G = R T l n K c

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Δ G^{0} = R T l n K c

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- Δ G^{0} = R T l n K c

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Solution

The correct option is D $- Δ G^{0} = R T l n K c$
The relationship between standard Gibbs energy change for a reaction and its equilibrium constant is ${Δ G}^{0} = - R T l n K_{c}$ or $- {Δ G}^{0} = R T l n K_{c} .$

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