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The oxidation of glucose to CO2 and H₂O is highly exergonic: AG = -636 kcal/mole. Why doesn't glucose spontaneously combust? O The glucose molecules lack the activation energy at room temperature. O There is too much CO₂ in the air. O CO₂ has higher energy than glucose. O The formation of six CO2 molecules from one glucose molecule decreases entropy. O The water molecules quench the reaction.

The oxidation of glucose to CO2 and H₂O is highly exergonic: AG = -636 kcal/mole. Why doesn't glucose spontaneously combust? O The glucose molecules lack the activation energy at room temperature. O There is too much CO₂ in the air. O CO₂ has higher energy than glucose. O The formation of six CO2 molecules from one glucose molecule decreases entropy. O The water molecules quench the reaction.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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The oxidation of glucose to CO2 and H₂O is highly exergonic: AG = -636 kcal/mole. Why doesn't glucose spontaneously combust? O The glucose molecules lack the activation energy at room temperature. O There is too much CO₂ in the air. O CO₂ has higher energy than glucose. O The formation of six CO2 molecules from one glucose molecule decreases entropy. O The water molecules quench the reaction.
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