The standard change in Gibbs free energy (ΔG°) can be calculated from the standard enthalpy change (ΔH°) and the standard entropy change (ΔS°). If ΔG° is negative, the reaction is expected to be spontaneous under standard conditions.
The standard change in Gibbs free energy (ΔG°) can be calculated from the standard enthalpy change (ΔH°) and the standard entropy change (ΔS°) using the equation ΔG° = ΔH° - TΔS°. The standard change in Gibbs free energy represents the change in free energy when one substance or set of substances in their standard states is converted to one or more other substances, also in their standard states.
In order to calculate ΔG°, you will need to know the values of ΔH° and ΔS° for the reaction. Once you have these values, you can substitute them into the equation and solve for ΔG°.
If the value of ΔG° is negative, the reaction is expected to be spontaneous under standard conditions. If the value of ΔG° is positive, the reaction is not expected to be spontaneous under standard conditions.