Discussion
The feasibility of a biochemical reaction is decided by the equation ΔG = ΔH-TΔS. If both ΔH and ΔS have negative values, the reaction :
Answer: C
The reaction is exergonic, favoured below T = ΔH/ΔS.
A reaction is spontaneous when \(\Delta G \lt 0\). With \(\Delta H \lt 0\) and \(\Delta S \lt 0\), the term \(-T\Delta S\) is positive and grows with temperature:
\[ \begin{aligned} \Delta G &= \Delta H - T\Delta S \lt 0 \\ T\Delta S &\gt \Delta H \\ T &\lt \frac{\Delta H}{\Delta S} \end{aligned} \]
The inequality flips at the last step because \(\Delta S\) is negative. So the favourable enthalpy wins at low temperature, and the reaction is exergonic and favoured below that temperature. It is not unfavoured at every temperature, it is not spontaneous at every temperature, and 'endergonic above' describes the opposite case of positive \(\Delta H\) and \(\Delta S\).
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