The Gibbs Free Energy at 298 K, AH = 46 kJ/mol and sº = 0.097 kJ/(K-mol) is 28.906 kJ/mol
It serves as the single master variable that determines whether a given chemical change is thermodynamically possible.
Thus if the free energy of the reactants is greater than that of the products, the entropy of the world will increase when the reaction takes place as written, and so the reaction will tend to take place spontaneously.
Conversely, if the free energy of the products exceeds that of the reactants, then the reaction will not take place in the direction written, but it will tend to proceed in the reverse direction.
At 298 K,
AH = 46 kJ/mol
and sº = 0.097 kJ/(K-mol).
ΔG=ΔH−T⋅ΔS
ΔG = 46 - 298 * 0.097
ΔG = 46 - 28.906
ΔG = 28.906 kJ/mol
The Gibbs Free Energy at 298 K, AH = 46 kJ/mol and sº = 0.097 kJ/(K-mol) is 28.906 kJ/mol
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