Gibbs Free Energy

Question

For a reaction to be spontaneous at all temperatures, which condition must be satisfied?

RankGuru · Accepted Answer

Spontaneity is determined by the **Gibbs Free Energy** change: $\Delta G = \Delta H - T\Delta S$.
For a reaction to be **spontaneous**, $\Delta G$ must be **negative**.
- If $\Delta H < 0$ (Exothermic) and $\Delta S > 0$ (Increased entropy), then:
$\Delta G = (-ve) - T(+ve)$.
- Since $T$ (absolute temperature) is always positive, $\Delta G$ will be negative **at any temperature**. This ensures spontaneity under all conditions.

Gibbs Free Energy

Select the correct option:

🔒 Solution Hidden from View

More chemical thermodynamics Practice Questions

At 298 K, a reaction has ΔH = +25 kJ mol⁻¹ and ΔS = +120 J mol⁻¹ K⁻¹. Is the reaction spontaneous at...

The relationship between Gibbs free energy change and cell potential is:

About This Question

Solution