For a given reaction with δδh = -26. 9 kj/mol, the δδg = 0 at 394 k. the value of δδs must be -68.27, using the equation ΔG=ΔH−TΔS.
Enthalpy and entropy are combined into a single quantity known as Gibbs free energy, or G. The product of the system's temperature and entropy, added to the enthalpy, equals the change in free energy, or G. ΔG=ΔH−TΔS is the equation for thermodynamics, where G represents the reaction's free energy. The change in entropy and free energy is what determines whether a reaction is spontaneous. The reaction will be spontaneous if there is an increase in entropy and a net decrease in free energy in the products.
As we know that,
ΔG=ΔH−TΔS
ΔH−TΔS = 0
ΔH = TΔS
-26900 = 394×ΔS
ΔS = -68.27
The change in entropy is negative as the system's unpredictability decreases.
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