ΔH = −100 kJ/mol, ΔS = −150 J/(mol·K), T = 298 K. ΔG ≈

−55 kJ/mol ΔG = −100 − 298(−0.150) = −100 + 44.7 ≈ −55 kJ/mol.

Gibbs Free Energy and Thermodynamic Favorability

AP Chemistry· difficulty 3/5

ΔH = -100 kJ/mol, ΔS = -150 J/(mol\cdotK), T = 298 K. ΔG \approx

Explanation

ΔG = -100 - 298(-0.150) = -100 + 44.7 \approx -55 kJ/mol.

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