# Relationship between equilibrium constant K, reaction quotient Q and Gibbs energy G 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, G 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

• If ΔG0 &lt; 0, then –ΔG0/RT is positive, and e-ΔG⁰ /RT &gt;1, making K &gt;1, which implies a spontaneous reaction or the reaction which proceeds in the forward direction to such an extent that the products are present predominantly.
• If ΔG0 &gt; 0, then –ΔG0/RT is negative, and e-ΔG⁰ /RT &lt; 1, that is, K &lt; 1, which implies a non-spontaneous reaction or a reaction which proceeds in the forward direction to such a small degree that only a very minute quantity of product is formed.