Question

ΔH° is -58.03 kJ and ΔS° is -176.6J/K. What is the value of ΔG° at 298K? Is the reaction spontaneous?

Answer 1

Solution.

∆G⁰=∆H⁰-T∆S⁰.

∆S⁰= -176,6 J/K= -0,1766 kJ/K.

∆G⁰₂₉₈= -58,03-298*(-0,1766) =-5,4032 kJ.

Since ∆G⁰₂₉₈< 0 the reaction is spontaneous.

Answer: ∆G⁰₂₉₈ = -5,4032 kJ. The reaction is spontaneous.