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onsider the following balanced equation for a redox reaction in an electrochemi ell: 3 Cd (s) + 2 NO3 (aq) + 8 H* (aq) → 3 Cd²* (aq) + 2 NO(g) + 4 H2O (1) E°. cell = 1.36 V Calculate the value of pH of the solution containing H*(ag) when the nonstandard c potential (Ecel) is measured to be 1.12 V given the following conditions at 25 °C: [NO] = 0.15 M; [Cd2*] = 0.46 M; PNo = 0.28 bar

onsider the following balanced equation for a redox reaction in an electrochemi ell: 3 Cd (s) + 2 NO3 (aq) + 8 H* (aq) → 3 Cd²* (aq) + 2 NO(g) + 4 H2O (1) E°. cell = 1.36 V Calculate the value of pH of the solution containing H*(ag) when the nonstandard c potential (Ecel) is measured to be 1.12 V given the following conditions at 25 °C: [NO] = 0.15 M; [Cd2*] = 0.46 M; PNo = 0.28 bar

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
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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Consider the following balanced equation for a redox reaction in an electrochemical cell: 3 Cd (s) + 2 NO3 (aq) + 8 H* (aq) → 3 Cd²+ (aq) + 2 NO(g) + 4H2O (1I) E°cell = 1.36 V Calculate the value of pH of the solution containing H*(aq) when the nonstandard cell potential (Ecell) is measured to be 1.12 V given the following conditions at 25 °C: [NO3] = 0.15 M; [Cd²+] = 0.46 M; PNO = 0.28 bar %3D %3D
Transcribed Image Text:Consider the following balanced equation for a redox reaction in an electrochemical cell: 3 Cd (s) + 2 NO3 (aq) + 8 H* (aq) → 3 Cd²+ (aq) + 2 NO(g) + 4H2O (1I) E°cell = 1.36 V Calculate the value of pH of the solution containing H*(aq) when the nonstandard cell potential (Ecell) is measured to be 1.12 V given the following conditions at 25 °C: [NO3] = 0.15 M; [Cd²+] = 0.46 M; PNO = 0.28 bar %3D %3D
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