Find the Temperature in Gibbs Free Energy

ΔG = ΔH – TΔS
ΔG = 178.2 – (373 x 160.6)/1000
ΔG = 178.2 – 59.9038
ΔG = 118.3 kJ mol-1

Find what temperature is required for the reaction to be spontanious

Thanks

For reaction to be spontaneous, ΔG must be less than zero.

Set up the equation:

ΔG = ΔH – TΔS ==> T = (ΔH - ΔG)/ΔS

ΔH = 278.2 kJ/mol
ΔG < 0
ΔS = 160.6 J/mol-K = 0.1606 kJ/mol-K

T > (278.2 - 0) / 0.1606

T > 1732 K

Using 4 significant digits:

Answer: Temperature = 1733 K