Question

If Qc>Kc then there will be a net backward reaction but still forward reaction will take place. My problem is if Qc>Kc forward reaction will become non spontaneous right. So how can that happen, does it like the gibbs free energy which released during backward reaction absorbs by products for forward reaction?

Answer 1

When Qc>Kc, the net direction of the reaction is backward, but forward reactions still occur as the system moves toward equilibrium, where both forward and reverse reactions occur at equal rates.

Step-by-step explanation:

If Qc>Kc, it indicates that the concentrations of the products are greater than what would be present at equilibrium, and thus the reaction will proceed in the reverse direction to reach equilibrium.

However, this does not mean that the forward reaction stops occurring. Chemical reactions are dynamic processes where both the forward and reverse reactions continue to occur, but when Qc>Kc, the net reaction is in the backward direction.

This is consistent with the principle that reactions tend toward equilibrium, where the forward and reverse reaction rates are equal. The relationship between the reaction quotient (Q), the equilibrium constant (K), and Gibbs free energy (ΔG) dictates the spontaneity of the reaction.

A positive ΔG indicates that the reaction is non-spontaneous in the forward direction but potentially spontaneous in the reverse direction until equilibrium is reached.