Question

1) What is the value of G at 120.0 K for a reaction in which H = +35 kJ/mol and S = 1.50

kJ/(mol.K)?

Answer 1

ΔG = -145kJ/mol

Step-by-step explanation:

To solve this question we must use the change in Gibbs free energy:

ΔG = ΔH - TΔS

Where ΔG is change in Gibbs free energy = ?

ΔH is enthalpy change = +35kJ/mol

T is absolute temperature = 120.0K

And ΔS is change in entropy = 1.50kJ/molK

Replacing:

ΔG = 35kJ/mol - 120.0K*1.50kJ/molK

ΔG = 35kJ/mol - 180kJ/mol

ΔG = -145kJ/mol