Determine the standard Gibbs free energy change, Δr G^∘, for the reactions of liquid methanol, o

step 1 Continuing to look at some of the basic parameters related to thermodynamics, here we're looking

Determine the standard Gibbs free energy change, Δr G^∘, for...

Determine the standard Gibbs free energy change, $\Delta_{\mathrm{r}} G^{\circ},$ for the reactions of liquid methanol, of $\mathrm{CO}(\mathrm{g}),$ and of ethyne, $\mathrm{C}_{2} \mathrm{H}_{2}(\mathrm{~g})$, with oxygen gas to form gaseous carbon dioxide and (if hydrogen is present) liquid water at $298 \mathrm{~K}$. Use your calculations to decide which of these substances are kinetically stable and which are thermodynamically stable: $\mathrm{CH}_{3} \mathrm{OH}(\ell), \mathrm{CO}(\mathrm{g}), \mathrm{C}_{2} \mathrm{H}_{2}(\mathrm{~g}), \mathrm{CO}_{2}(\mathrm{~g})$ $\mathrm{H}_{2} \mathrm{O}(\ell)$

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Key Concepts

Standard Gibbs Free Energy Change

This is a thermodynamic quantity that indicates the spontaneity of a chemical reaction under standard conditions. It is calculated using the standard free energies of formation of reactants and products and reflects the overall energy change associated with a reaction. A negative standard Gibbs free energy change implies that the reaction is thermodynamically favorable, while a positive value indicates non-spontaneity under standard conditions.

Thermodynamic Stability

Thermodynamic stability refers to the inherent energy state of a substance, where a thermodynamically stable substance is one that has a low free energy and is less likely to undergo a spontaneous reaction. In the context of combustion or oxidation reactions, a molecule that forms products with significantly lower free energy compared to the reactants is considered thermodynamically unstable.

Kinetic Stability

Kinetic stability describes the rate at which a reaction proceeds, which is determined by the activation energy barrier rather than the overall free energy change. A substance can be thermodynamically unstable (favorable reaction in energy terms) but still persist because the reaction has a high activation barrier, making it react very slowly unless an appropriate catalyst or extreme conditions are provided.

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