Question

According to the Gibbs free energy equation, G= H-T S, when could a high temperature make a reaction that was nonspontaneous at low temperature spontaneous

Answer 1

When ΔH and ΔS are both positive

Answer 2

For the reaction to be spontaneous at high temperatures, ΔG < 0 and, ΔH > 0 and ΔS > 0.

Step-by-step explanation:

According to the Gibbs free energy equation, for the reaction to be spontaneous at high temperatures when it was not spontaneous at low temperatures, the free energy change ΔG < 0.

Since ΔG = ΔH - TΔS where ΔH = enthalpy change and ΔS = entropy change,

For ΔG < 0 at high temperatures, ΔH > 0 and ΔS > 0. That is both ΔH and ΔS are positive at high temperatures.

So, for the reaction to be spontaneous at high temperatures, ΔG < 0, and ΔH > 0 and ΔS > 0.