The oxidation of NH4+ to NO3- in acid solution (pH = 5.600) is described by the following equation: $$ The overall reaction for the oxidation has an E\deg cell = -0.2710 V. E\deg = 1.50 V for the half-reaction $$ 2nd attempt See Hint Be sure to solve the equation using a base-10 logarithm (log) rather than the natural logarithm (In ). What is the ratio of [NO3-] to [NH4+] at 298 K if PO2 = 0.180 atm? Assume that the reaction is at equilibrium.

The oxidation of NH4+ to NO3- in acid solution (pH = 5.600) is described by the following equation: $$ The overall reaction for the oxidation has an E\deg cell = -0.2710 V. E\deg = 1.50 V for the half-reaction $$ 2nd attempt See Hint Be sure to solve the equation using a base-10 logarithm (log) rather than the natural logarithm (In ). What is the ratio of [NO3-] to [NH4+] at 298 K if PO2 = 0.180 atm? Assume that the reaction is at equilibrium.

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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