For the cell shown, the measured cell potential, \( E_{\text{cell}} \), is \(-0.3575 \, \text{V}\) at \(25^\circ \text{C}\).\[\text{Pt(s) | H}_2 \text{(g, 0.793 atm) | H}^+ \text{(aq, ? M) || Cd}^{2+} \text{(aq, 1.00 M) | Cd(s)}\]The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, \( E^\circ \), are\[\text{2 H}^+ \text{(aq) + 2 e}^- \rightarrow \text{H}_2 \text{(g)} \quad E^\circ = 0.00 \, \text{V}\]\[\text{Cd}^{2+} \text{(aq) + 2 e}^- \rightarrow \text{Cd(s)} \quad E^\circ = -0.403 \, \text{V}\]Calculate the \( \text{H}^+ \) concentration.\[[\text{H}^+] = \, \_\_\_\_\_\_\_\_\_\_ \, \text{M}\]There is a box labeled "TOOLS" with \( \times 10^y \) indicating the option to input the power of ten for the hydrogen ion concentration.

Answered: Image /qna-images/answer/2f09bf99-31fd-4583-80b3-3e42911f9d80.jpg

o For the cell shown, the measured cell potential, Ecell, is -0.3575 V at 25 °C. Pt(s) | H₂(g,0.793 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, Eº, are 2 H+ (aq) + 2e → H₂(g) Cd² (aq) + 2e → Cd(s) Calculate the H+ concentration. [H+] = x10 TOOLS E° = 0.00 V E° = -0.403 V M Attempt

o For the cell shown, the measured cell potential, Ecell, is -0.3575 V at 25 °C. Pt(s) | H₂(g,0.793 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, Eº, are 2 H+ (aq) + 2e → H₂(g) Cd² (aq) + 2e → Cd(s) Calculate the H+ concentration. [H+] = x10 TOOLS E° = 0.00 V E° = -0.403 V M Attempt

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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