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We know that a reaction with delta G < 0, favors the forward direction, towards products....

We know that a reaction with delta G < 0, favors the forward direction, towards products. However, it does not guarantee that the process will immediately occur. Why not? What factor relate to rate of reaction?

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Answer #1

entrophy is the other factor to decide spontinity of the reaction .

ΔG = ΔH - TΔS , ΔG is change in the free energy, ΔH is the change in enthalpy, ΔS is the change in entropy and T is temperature in kelvin.

When ΔH is negative and ΔS is positive, ΔG will be negative over all temperatures.

When ΔH is negative and ΔS is negative, ΔG will be negative at low temperatures.

When ΔH is positive and ΔS is negative, ΔG will not be negative at any temperature. There would be no spontaneous reaction.

When ΔH is positive and ΔS is positive, ΔG will be negative at high temperatures.

Therefore, finally it is the change in free energy of a reaction which can predict if a reaction is feasible.

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