Which of the following statements about the combustion of glucose with oxygen to form water and carbon dioxide $\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}+6 \mathrm{O}_{2}-6 \mathrm{CO}_{2}+6 \mathrm{H}_{2} \mathrm{O}\right)$ is correct?
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The entropy of the universe decreases as the result of this reaction.
This is the process of cellular respiration, an anabolic pathway that releases free energy.
The free energy lost in this combustion is less than the energy that appears as heat.
The reverse reaction, making glucose from water and carbon dioxide, must be an exergonic reaction.
The entropy of the products is greater than the entropy of the reactants.

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Accepted Answer

***E*** ∻Key Concept∻ ⚹Entropy⚹ ∻Explanation∻ ⚹In the combustion of glucose, the entropy of the products (CO₂ and H₂O) is greater than the entropy of the reactants (C₆H₁₂O₆ and O₂). This is because the reaction results in an increase in the number of molecules and the dispersal of energy.⚹◊What is the overall balanced chemical equation for the combustion of glucose with oxygen to form water and carbon dioxide?⍭ Generate me a similar question◊

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