Consider the cell notation: Zn/Zn2+(0.0364 M) // Tl+3(9.00x10-3 M) , Tl+(0.0620 M) /Pt at 298 K.Write the balanced electrochemical reaction involved.What is the Eºcell? Given the standard reduction potential values: Eºred Zn+2/Zn = -0.403 V and Eºred Tl+3/Tl+= 1.25 V. Use the actual molar concentrations of the ions in the cell notation and determine the cell potential.

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Answered: Write the balanced electrochemical…

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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Consider the cell notation: Zn/Zn2+(0.0364 M) // Tl+3(9.00x10-3 M) , Tl+(0.0620 M) /Pt at 298 K.

Write the balanced electrochemical reaction involved.
What is the Eºcell? Given the standard reduction potential values: Eºred Zn+2/Zn = -0.403 V and Eºred Tl+3/Tl+= 1.25 V.
Use the actual molar concentrations of the ions in the cell notation and determine the cell potential.

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