Calculate the expected Ecell for each galvanic cells.Reduction potential of Zn2+(0.1 M)/Zn half-cell: –0.79 VProcedurePipet 1 mL of the 0.1 M Cu(NO3)2 solution (Solution 1) from the Zn2+(0.1 M)/Zn half-cell into a 50 mL volumetric flask and dilute to the mark with deionized water. Pour this diluted solution (Solution 2) into a 50 mL beaker.Pipet 1 mL of Solution 2 into a 50 mL volumetric flask and dilute to the mark with deionized water. Pour this diluted solution (Solution 3) into a 50 mL beaker. Repeat using Solution 3 to prepare Solution 4. Measure the cell potential for each of the three galvanic cells that can be made by pairing the Zn2+(0.1 M)/Zn half-cell with the half-cells containing Solutions 2–4 and the copper electrode.

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Answered: Calculate the expected Ecell for each…

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 111QRT

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Calculate the expected Ecell for each galvanic cells.

Reduction potential of Zn2+(0.1 M)/Zn half-cell: –0.79 V

Procedure

Pipet 1 mL of the 0.1 M Cu(NO3)2 solution (Solution 1) from the Zn²⁺(0.1 M)/Zn half-cell into a 50 mL volumetric flask and dilute to the mark with deionized water. Pour this diluted solution (Solution 2) into a 50 mL beaker.
Pipet 1 mL of Solution 2 into a 50 mL volumetric flask and dilute to the mark with deionized water. Pour this diluted solution (Solution 3) into a 50 mL beaker. Repeat using Solution 3 to prepare Solution 4.
Measure the cell potential for each of the three galvanic cells that can be made by pairing the Zn²⁺(0.1 M)/Zn half-cell with the half-cells containing Solutions 2–4 and the copper electrode.

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