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Using the following electrode potentials, determine the redox potential for the oxidation of nitrite ions (NO,) to nitrate ions (NO3). NO3 → NO2 E° = 0.94 V 02→ H20 E° = 1.23 V Select one: а. +0.65 V b. +0.29 V с. -0.29 V d. -0.65 V е. +2.17 V

Using the following electrode potentials, determine the redox potential for the oxidation of nitrite ions (NO,) to nitrate ions (NO3). NO3 → NO2 E° = 0.94 V 02→ H20 E° = 1.23 V Select one: а. +0.65 V b. +0.29 V с. -0.29 V d. -0.65 V е. +2.17 V

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.44QE: For each of the reactions, calculate E from the table of standard potentials, and state whether the...
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Using the following electrode potentials, determine the redox potential for the oxidation of nitrite ions (NO2) to nitrate ions (NO3). NO3 NO2 E° = 0.94 V 02- H20 E° = 1.23 V Select one: а. +0.65 V b. +0.29 V С. -0.29 V O d. -0.65 V е. +2.17 V
Transcribed Image Text:Using the following electrode potentials, determine the redox potential for the oxidation of nitrite ions (NO2) to nitrate ions (NO3). NO3 NO2 E° = 0.94 V 02- H20 E° = 1.23 V Select one: а. +0.65 V b. +0.29 V С. -0.29 V O d. -0.65 V е. +2.17 V
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