The oxidation of glucose to CO2 and H2O is highly exergonic: δg of -636 kcal/mol. This is spontaneous, but with such a high magnitude of free energy difference, why is it very slow?

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11-08-2022
Chemistry

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The oxidation of glucose to CO2 and H2O is highly exergonic: δg of -636 kcal/mol. This is spontaneous, but with such a high magnitude of free energy difference, why is it very slow?

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tripatsingh039 tripatsingh039 · Answer 1 · 2022-08-17T06:26:54+02:00

Glucose reacts with molecular oxygen to produce carbon dioxide and water. The carbon atoms in glucose are oxidized. That is, they lose electron and go to a higher oxidation state. The oxygen atoms in molecular oxygen are reduced.

A spontaneous chemical reaction occurs with no outside influence, and can be very fast or stretch over millions of years .Glucose is oxidized into 2 molecules of pyruvic acid in an exergonic reaction. We can use Gibbs free energy, ΔG, to determine if a reaction is spontaneous or not at a particular temperature. It is computed from the enthalpy change, ΔH, and the change in entropy, ΔS, and the absolute temperature. If ΔG has a negative sign, the reaction is spontaneous at temperature T.

ΔG = ΔH - TΔS

Learn more about Temperature here-

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