Consider the reaction 2 NOCl(g) $\rightarrow$ CL₂ (g) + 2 No(g), for which $\Delta$H $\degree$ = +77.2 kJ/mol and $\Delta$S $\degree$ =+121.0 J/mol . K.Which of the following statements regarding its temperature dependence is true?

Question

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The spontaneity of a reaction can be determined by the Gibbs free energy change ($\Delta G$), which is related to the enthalpy change ($\Delta H$) and the entropy change ($\Delta S$) of the reaction by the equation $\Delta G = \Delta H - T\Delta S$. Given that $\Delta H$ is positive (+77.2 kJ/mol) and $\Delta S$ is also positive (+121.0 J/mol·K), at low temperatures, the $T\Delta S$ term will be smaller, making $\Delta G$ positive (nonspontaneous). At high temperatures, the $T\Delta S$ term will increase, potentially making $\Delta G$ negative (spontaneous), indicating that the reaction becomes spontaneous as the temperature increases.

Consider the Reaction 2 NOCl(g) →\rightarrow→ CL2 (G) + 2 No(g), for Which

Consider the Reaction 2 NOCl(g) $\rightarrow$ CL₂ (G) + 2 No(g), for Which