If ∆G = ∆H - T∆S and T= 295K∆H= -92.22 kJ ∆S= -0.198 kJ/K What is ∆G

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30-10-2022
Chemistry

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If ∆G = ∆H - T∆S and T= 295K∆H= -92.22 kJ ∆S= -0.198 kJ/K What is ∆G

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OzF325066 OzF325066 · Answer 1 · 2022-10-30T13:43:09+01:00

The Gibbs free energy tells us the maximum amount of work that can be reversible in a closed system, that is, there is no input or output of matter. By thermodynamics, the Gibbs free energy can be related to the enthalpy and entropy of the system, all of them dependent on temperature, so we have the following relationship:

[tex]\Delta G=\Delta H-T\Delta S[/tex]

Now, since we have the values of enthalpy, entropy, and the temperature of the system we plug these values into the equation.

[tex]\begin{gathered} \Delta G=-92.22kJ-295K\times(-0.198kJ/K) \\ \Delta G=-92.22kJ+58.41kJ=-33.81kJ \end{gathered}[/tex]

So, the deltaG has a value of -33.81kJ, has a negative value.

A negative Gibbs free energy means that the reactants or initial state have more free energy than the products or final state, and the process will be spontaneous.

Answer: ∆G= - 33.81kJ