I keep getting “Gibbs free energy” questions wrong in Chemical Thermodynamics. What's the trap?
judging spontaneity from ΔH alone.
The usual trap: judging spontaneity from ΔH alone. How to avoid it: an endothermic reaction can still be spontaneous if TΔS is large enough. Go back to the definition — ΔG = ΔH − TΔS decides spontaneity — negative ΔG means the process is spontaneous.
Key point
Gibbs free energy
Common mistake
judging spontaneity from ΔH alone.
Memory tip
an endothermic reaction can still be spontaneous if TΔS is large enough.
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