Question

Calculate the change in Gibbs free energy for each of the following sets of ΔH∘rxn, ΔS∘rxn, and T.

a. ΔH∘rxn=− 126 kJ ; ΔS∘rxn= 255 J/K ; T= 294 K

b. ΔH∘rxn= 126 kJ ; ΔS∘rxn=− 255 J/K ; T= 294 K

c. ΔH∘rxn=− 126 kJ ; ΔS∘rxn=− 255 J/K ; T= 294 K

d. ΔH∘rxn=− 126 kJ ; ΔS∘rxn=− 255 J/K ; T= 557 K

I'm super confused on these. Any help would be appreciated, thank you.

Answer 1

The formula of Gibbs free energy given as follows

∆G° = ∆H° -T∆S° .......(1)

Where,

∆G ° = standard Gibbs free energy

∆H° = standard enthalpy

T = temperature

∆S° = standard entropy

And

1j = 10^-3kJ