3. Standard reduction potentials are listed for reactions under standard conditions. Standard conditions are 1 M concentrations of ions, I atm (or 1 bar) partial pressures for gases, and a temperature of 298 K. In Part I. you were asked to compare your measured cell potential to a calculated standard cell potential. The cell potential you measured was for a galvanic cell you prepared using 0.10 M solutions of Pb²* and Cu, not 1.0 M solutions, Write out the balanced equation for this cell, then give the Nernst equation for this cell. From the Nernst equation, explain why the cell potential under these nonstandard conditions should be equal to the standard cell potential for this particular reaction. a.
3. Standard reduction potentials are listed for reactions under standard conditions. Standard conditions are 1 M concentrations of ions, I atm (or 1 bar) partial pressures for gases, and a temperature of 298 K. In Part I. you were asked to compare your measured cell potential to a calculated standard cell potential. The cell potential you measured was for a galvanic cell you prepared using 0.10 M solutions of Pb²* and Cu, not 1.0 M solutions, Write out the balanced equation for this cell, then give the Nernst equation for this cell. From the Nernst equation, explain why the cell potential under these nonstandard conditions should be equal to the standard cell potential for this particular reaction. a.
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter17: Electrochemistry
Section: Chapter Questions
Problem 59P
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