For the cell shown, the measured cell potential, Ecell, is −0.3657 V at 25 °C.Feedback×Pt(s) | H₂(g, 0.777 atm) | H+ (aq, ? M) || Cd²+ (aq, 1.00 M) | Cd(s)Remember that Q is equal to theconcentration or partial pressure of theThe balanced reduction half-reactions for the cell, and their respective standard reduction potential values, products raised to the power of theircoefficients in the balanced equation,2 H+ (aq) + 2 e¯H₂(g)Eº = 0.00 VCd²+ (aq) + 2e → Cd(s)Eº = -0.403 VCalculate the H+ concentration.divided by the concentration or partialpressure of the reactants raised to thepower of their coefficients in thebalanced equation. Because there aretwo moles of H+ in the balancedreaction, the superscript on [H+] in theQ expression should be 2.0.0425[H+]Incorrect

Given-> 2H+(aq) + 2e- ------> H2(g) E°= 0.00 V Cd2+(aq) + 2e- -------> Cd(s) E°= -0.403 V…

For the cell shown, the measured cell potential, Ecell, is -0.3657 V at 25 °C. Pt(s) | H₂(g, 0.777 atm) | H+ (aq, ? M) || Cd²+ (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, 2 H+ (aq) + 2e H₂(g) Eº = 0.00 V Cd²+ (aq) + 2 e → Cd(s) E° -0.403 V = Calculate the H+ concentration. 0.0425 [H+] = Incorrect

For the cell shown, the measured cell potential, Ecell, is -0.3657 V at 25 °C. Pt(s) | H₂(g, 0.777 atm) | H+ (aq, ? M) || Cd²+ (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, 2 H+ (aq) + 2e H₂(g) Eº = 0.00 V Cd²+ (aq) + 2 e → Cd(s) E° -0.403 V = Calculate the H+ concentration. 0.0425 [H+] = Incorrect

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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