1. Calculate E for the following electrochemical cell at 25 °C Pt(s) | H2(g, 1.00 atm)| H*(aq, 1.00 M) || Cu²*(aq, 0.315 M)| Cu(s) given the following standard reduction potentials. Cu2*(aq) + 2 e – Cu(s) E° = +0.337 V 2 H*(aq) + 2 e – H2(g) E° = 0.000 V

1. Calculate E for the following electrochemical cell at 25 °C Pt(s) | H2(g, 1.00 atm)| H(aq, 1.00 M) || Cu²(aq, 0.315 M)| Cu(s) given the following standard reduction potentials. Cu2(aq) + 2 e – Cu(s) E° = +0.337 V 2 H(aq) + 2 e – H2(g) E° = 0.000 V

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 50QRT

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The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.
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