A reaction has a ΔH°= 204.6 kJ and a ΔS°= -19.5 J/K. a. Given the sign...

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A reaction has a ΔH°= 204.6 kJ and a ΔS°= -19.5 J/K. a. Given the sign...

A reaction has a ΔH°= 204.6 kJ and a ΔS°= -19.5 J/K.

a. Given the sign and magnitude of ΔH and ΔS, will the reaction be spontaneous at all temperatures, nonspontaneous at all temperatures? Briefly explain your reasoning.

b. Calculate the standard free energy change for the reaction at 298 K.
c. Is the reaction spontaneous or nonspontaneous at 298 K?

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Answer 1

Answer #1

+ Given ; AH = 204.6 kJ ASO = - 19.5 J/K (a) - According to thermodynamics. AG = AM - TASO & If AGO 20 Reaction is spontaneou

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Answer 2

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A reaction has a ΔH°= 204.6 kJ and a ΔS°= -19.5 J/K. a. Given the sign...

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A reaction has a ΔH°= 204.6 kJ and a ΔS°= -19.5 J/K. a. Given the sign...