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Consider two redox half reactions, one in which glucose is oxidized (to CO2), and another in which palmitate is oxidized (to CO2). For both oxidation reactions, O2 is used as the terminal electron acceptor and reduced to H2O. The half reaction involving glucose has a known redox potential (E’o = -0.43 V). The redox potential for the oxidation of palmitate to CO2 does not. Would the redox potential (E’o) of the half reaction involving palmitate oxidation to CO2 be higher or lower than that of glucose oxidation to CO2? Explain your reasonin

Consider two redox half reactions, one in which glucose is oxidized (to CO2), and another in which palmitate is oxidized (to CO2). For both oxidation reactions, O2 is used as the terminal electron acceptor and reduced to H2O. The half reaction involving glucose has a known redox potential (E’o = -0.43 V). The redox potential for the oxidation of palmitate to CO2 does not. Would the redox potential (E’o) of the half reaction involving palmitate oxidation to CO2 be higher or lower than that of glucose oxidation to CO2? Explain your reasonin

Chemistry
Chemistry
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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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Consider two redox half reactions, one in which glucose is oxidized (to CO2), and another in which palmitate is oxidized (to CO2). For both oxidation reactions, O2 is used as the terminal electron acceptor and reduced to H2O. The half reaction involving glucose has a known redox potential (E’o = -0.43 V). The redox potential for the oxidation of palmitate to CO2 does not.

Would the redox potential (E’o) of the half reaction involving palmitate oxidation to CO2 be higher or lower than that of glucose oxidation to CO2? Explain your reasoning.

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