The Gibbs energy change during mixing contributes which component for two gases?

In the context of mixing two gases, the Gibbs energy change is influenced by both the enthalpy and entropy of the system. When two different gases are mixed, there are energetic interactions to consider, which pertain to enthalpy. If the process of mixing is exothermic, it typically indicates that the enthalpy component is favorable.

At the same time, mixing increases the disorder or randomness of the system, which corresponds to an increase in entropy. The greater the randomness, the more favorable the mixing process becomes. This increase in entropy often drives the spontaneity of the mixing process, even if the overall enthalpy change is not strongly negative.

Thus, for mixing two gases, the Gibbs energy change indeed involves contributions from both enthalpy and entropy. This is because the Gibbs free energy equation (( \Delta G = \Delta H - T\Delta S )) illustrates how changes in enthalpy and entropy together determine the overall change in Gibbs energy during a mixing process. The correct response highlights the dual role of enthalpy and entropy in this context, making it clear that both factors are essential in understanding the mixing behavior of gases.