For a particular reaction, ΔH° is -46.7 kJ/mol and ΔS° is -123.8 J/(mol·K). Assuming these values change very l

Question

Anybody able to help and explain this problem?

For a particular reaction, ΔH° is -46.7 kJ/mol and ΔS° is -123.8 J/(mol·K). Assuming these values change very little with temperature, over what temperature range is the reaction spontaneous in the forward direction?

Answer 1

To be spontaneous in the forward direction, you need ΔG < 0 (Gibbs free energy moves toward minimum as you approach equilibrium.)

 

ΔG = ΔH - TΔS

 

Since you are given ΔH and ΔS, you can solve for the range of T that makes ΔG < 0.