Question

derive the relationship between equilibrium constant k , reaction quotient q and gibb's free energy
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Answer 1

Answer:

Relationship between equilibrium constant K, reaction quotient Q and Gibbs energy G. ... ΔG is negative, then the reaction is spontaneous and proceeds in the forward direction. ΔG is positive, then reaction is considered non-spontaneous. Instead, as reverse reaction would take place.

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Answer 2

Answer:

We know that if,

ΔG is negative, then the reaction is spontaneous and proceeds in the forward direction.

ΔG is positive, then reaction is considered non-spontaneous. Instead, as reverse reaction would take place

ΔG is 0, reaction has achieved equilibrium; at this point, there is no longer any free energy left to drive the reaction.

A mathematical expression of this thermodynamic view of equilibrium can be described by the following equation:

ΔG = ΔG⁰ + RT ln Q

Where, G⁰ is standard Gibbs energy.

At equilibrium, when ΔG = 0 and Q = Kc

ΔG = ΔG⁰ + RT ln K = 0

ΔG⁰ = -RT ln K

ln K = ΔG⁰ / RT

Taking antilog of both sides, we get,

K = e-ΔG⁰ /RT

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