If $ \Delta G = 0 $: The system is at equilibrium.
If $ \Delta G > 0 $: The process is non-spontaneous under the given conditions.
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Which combination of signs for ΔH and ΔS corresponds to a reaction that is spontaneous only at low temperatures?
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What is the Gibbs free energy equation?
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Introduction to Gibbs Free Energy
Gibbs Free Energy is a thermodynamic potential that helps predict whether a process will occur spontaneously.
It combines three fundamental concepts: enthalpy (ΔH), entropy (ΔS), and temperature (T).
The formula is given by: ΔG=ΔH−TΔS
AnalogyThink of Gibbs Free Energy as a bank account balance where:
ΔH is your income (energy input/output)
TΔS is your expenses (energy dispersal)
ΔG is your net savings (spontaneity)
DefinitionSpontaneous ProcessA process that occurs naturally without external intervention.
ExampleA ball rolling downhill is a spontaneous process, while pushing it uphill requires effort.
