For a particular reaction, Δ H ∘ = 20.1 kJ/mol and Δ S ∘ = 45.9 J / (mol ⋅ K). Assuming these values change very little with temperature,
at what temperature does the reaction change from nonspontaneous to spontaneous in the forward direction? T = K

438 K

Explanation:

According to Gibbs equation:

= Gibb's free energy change

= enthalpy change = 20.1 kJ/mol = 20100 J/mol

T = temperature

= entropy change = 45.9 J/Kmol

A reaction is at equilibrium when = Gibb's free energy change is zero and becomes spontaneous when = Gibb's free energy change is negative.

T=437.9K

Thus the temperature at which the reaction change from nonspontaneous to spontaneous in the forward direction is 438 K

i believe the answer is a.

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