Is it energetically favorable for nitrogen pentoxide to decompose at 350 K, where ΔH is 6000 J/mol and ΔS is 25 J/Kmol?

Answer 1

For the reaction to be energetically favorable, ∆G should be negative (spontaneous reaction). So, we will need to find the value of ∆G.

∆G = ∆H - T∆S

∆G = 6000 J / mol - (350K x 25 J/Kmol)

∆G = 6000 J / mol - 8750 J / mol

∆G = -2750 kJ/mol

Since ∆G is negative the reaction is favorable at 350K.