The answer for the following problem is mentioned below.
Therefore the Gibbs free energy (ΔG) for the reaction is -394.36 J
Explanation:
Given:
ΔH = -393.5 kJ/ mol
ΔS =0.0029 kJ/mol K
T = 298 K
To solve:
Gibbs free energy (ΔG)
We know;
ΔG = ΔH - TΔS
ΔG = -393.5 - (298 × 0.0029)
ΔG = -393.5 - 0.8642
ΔG = -394.36 J
Therefore the Gibbs free energy (ΔG) for the reaction is -394.36 J
