What will be the Gibbs free energy in KJ/mol if the entropy of the reaction (ΔS°rxn) is 342.26 KJ/mole and the ethlapy (ΔH°rxn) is -422.77 J/mol at 33.48 oC?
What will be the Gibbs free energy in KJ/mol if the entropy of the reaction (ΔS°rxn) is 342.26 KJ/mole and the ethlapy (ΔH°rxn) is -422.77 J/mol at 33.48 oC?
Chapter17: Spontaneity, Entropy, And Free Energy
Section: Chapter Questions
Problem 38E: For mercury, the enthalpy of vaporization is 58.51 kJ/mol and the entropy of vaporization is 92.92...
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What will be the Gibbs free energy in KJ/mol if the entropy of the reaction (ΔS°rxn) is 342.26 KJ/mole and the ethlapy (ΔH°rxn) is -422.77 J/mol at 33.48 oC?
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