Gibbs free energy change is a thermodynamic property that helps in determining the spontaneity and feasibility of a chemical reaction. It takes into account two important factors, namely enthalpy (ΔH) and entropy (ΔS). However, it does not depend on the number of moles of reacting species. Let's understand this concept in detail.

Enthalpy of reaction:

Enthalpy of reaction is the amount of heat energy released or absorbed during a chemical reaction. It is denoted by ΔH and is an important factor in determining the Gibbs free energy change. If the enthalpy change is negative, it means that the reaction is exothermic and the Gibbs free energy change will be negative, indicating a spontaneous reaction. On the other hand, if the enthalpy change is positive, it means that the reaction is endothermic and the Gibbs free energy change will be positive, indicating a non-spontaneous reaction.

Randomness of the molecules participating in reaction:

Entropy is a measure of randomness or disorder of a system. It is denoted by ΔS and is another important factor in determining the Gibbs free energy change. If the entropy change is positive, it means that the disorder of the system increases and the Gibbs free energy change will be negative, indicating a spontaneous reaction. On the other hand, if the entropy change is negative, it means that the disorder of the system decreases and the Gibbs free energy change will be positive, indicating a non-spontaneous reaction.

Number of moles of reacting species:

The number of moles of reacting species does not affect the Gibbs free energy change. This is because Gibbs free energy change is a state function and depends only on the initial and final states of the system, not on the path taken between them. Therefore, even if the number of moles of reacting species changes during the reaction, it does not affect the Gibbs free energy change.

Temperature of the reaction:

Temperature is also an important factor in determining the Gibbs free energy change. If the temperature is high, it means that the kinetic energy of the molecules increases, leading to an increase in the entropy of the system. This can make a non-spontaneous reaction spontaneous. On the other hand, if the temperature is low, it means that the kinetic energy of the molecules decreases, leading to a decrease in the entropy of the system. This can make a spontaneous reaction non-spontaneous.

In conclusion, Gibbs free energy change depends on enthalpy and entropy, but not on the number of moles of reacting species. It is also affected by the temperature of the reaction.