For the cell shown, the measured cell potential, ?cell, is −0.3553 V at 25 °C. Pt(s) | H2(g,0.803 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, ?o, are
For the cell shown, the measured cell potential, ?cell, is −0.3553 V at 25 °C. Pt(s) | H2(g,0.803 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, ?o, are
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.47QE
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For the cell shown, the measured cell potential, ?cell, is −0.3553 V at 25 °C.
Pt(s) | H2(g,0.803 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, ?o, are
2H+(aq)+2e−⟶H2(g) ?o=0.00 V
Cd2+(aq)+2e−⟶Cd(s)?o=−0.403 V
Calculate the H+ concentration.
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