Pb4+(aq) + 2e- <-> Pb2+(aq) ΔHfo = ΔGfo = 0 kJ/mol. ΔSfo = 68.85 J/mol-K. Calculate the cell voltage, E, at 25oC if the concentration of Pb4+ 0.5M and that of Pb2+ is 0.1M. Use the Nernst equation.
Pb4+(aq) + 2e- <-> Pb2+(aq) ΔHfo = ΔGfo = 0 kJ/mol. ΔSfo = 68.85 J/mol-K. Calculate the cell voltage, E, at 25oC if the concentration of Pb4+ 0.5M and that of Pb2+ is 0.1M. Use the Nernst equation.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter19: Principles Of Chemical Reactivity: Electron Transfer Reactions
Section19.5: Electrochemical Cells Under Nonstandard Conditions
Problem 19.7CYU: 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...
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Pb4+(aq) + 2e- <-> Pb2+(aq)
ΔHfo = ΔGfo = 0 kJ/mol. ΔSfo = 68.85 J/mol-K.
Calculate the cell voltage, E, at 25oC if the concentration of Pb4+ 0.5M and that of Pb2+ is 0.1M. Use the Nernst equation.
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