Answer is: temperature must be increased to very high values.
The change in
Gibbs free energy (ΔG), at constant temperature and pressure, is: ΔG=ΔH−TΔS.
ΔH is the change in enthalpy; in this example ΔH>0..
ΔS is change in entropy; ΔS>0.
T is temperature of the system.
When ΔG is negative, a reaction (occurs without the addition of
external energy) will be spontaneous (exergonic).
TΔS > ΔH.
