For the cell shown, the measured cell potential, Ecell, is –0.3601 V at 25 °C. Pt(s) | H, (g, 0.857 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, E°, are 2 H*(aq) + 2e¯ → H, (g) E° = 0.00 V Cd2+(aq) + 2 e¯ → Cd(s) E° = -0.403 V Calculate the H+ concentration.
For the cell shown, the measured cell potential, Ecell, is –0.3601 V at 25 °C. Pt(s) | H, (g, 0.857 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, E°, are 2 H*(aq) + 2e¯ → H, (g) E° = 0.00 V Cd2+(aq) + 2 e¯ → Cd(s) E° = -0.403 V Calculate the H+ concentration.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter17: Electrochemistry And Its Applications
Section: Chapter Questions
Problem 38QRT
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![For the cell shown, the measured cell potential, Ecell, is –0.3601 V at 25 °C.
Pt(s) | H, (g, 0.857 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, E°, are
2 H* (aq) + 2 e
H, (g)
Е® — 0.00 V
>
Cd²+(aq) + 2 e-
Cd(s)
E° = -0.403 V
Calculate the H+ concentration.
[H*] =
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faaf0ed00-66bd-42da-a6f7-e9e58a893ff0%2F1a3c6998-7a13-406d-b968-545f0fe7434e%2F41uxgn_processed.png&w=3840&q=75)
Transcribed Image Text:For the cell shown, the measured cell potential, Ecell, is –0.3601 V at 25 °C.
Pt(s) | H, (g, 0.857 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, E°, are
2 H* (aq) + 2 e
H, (g)
Е® — 0.00 V
>
Cd²+(aq) + 2 e-
Cd(s)
E° = -0.403 V
Calculate the H+ concentration.
[H*] =
M
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