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The oxidation of glucose to ${CO}_2$ and ${H}_{2}O$ has a Gibb's free energy value of $\Delta G=-$636 kcal/mol.

Why is it that the jar of glucose in your kitchen does not spontaneously convert into ${CO}_2$ and ${H}_{2}O$?

A

${CO}_2$ has more stored energy than glucose, therefore the reaction requires the input of 636 kcal/mol of energy to move forward.

B

The reaction require more oxygen than is provided for by normal atmospheric conditions.

C

The glucose molecules lack the activation energy at room temperature needed for the reaction to move forward.

D

There is too much ${CO}_2$ in the air and this hinders the production of more ${CO}_2$ from glucose.

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