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From the values of delta H and delta S, predict which of the following reactions would...

From the values of delta H and delta S, predict which of the following reactions would be spontaneous at 26C: Reaction A: delta H = 10.5 kJ/mol, delta S = 30.0 J/K*mol Reaction B: delta H = 1.8 kJ/mol, delta S = -113 J/K*mol If either of the reactions is nonspontaneous, can it (they) become spontaneous? If either of the reactions is nonspontaneous but can become spontaneous, at what temperature might it become spontaneous? Please explain how to do this!

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Answer #1

The relationship for the value of Gibbs Free energy (AG) is: AG-AH-TAS The AH is the change in enthalpy of the system and AS0 > 10.5 JÁnol-T (30.0) J/mol. K -1 0.5 kJ/mol>-T ( 0.030) kJ/mol . K 350<T Thus, the reaction A is spontaneous at temperatur

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