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2. In another cell, the potential of the copper metal, copper(II) ion electrode was found to be 0.442 V rela- tive to a silver metal, silver ion electrode, with the copper electrode being negative. Ag+, Ag a. If the potential of the silver, silver ion electrode, E is taken to be 0.000 V in oxidation or reduction, what is the value of the potential for the oxidation reaction, EC.Cu²+oxid? Ecell = Eoxid + Ered 0.00V=[ord #-0.442 Eoxid = 0.442 6,442 volts b. If E Ag.Ag red. equals +0.799V, as in standard tables of electrode potentials, what is the value of the potential of the oxidation reaction of copper, Ecu,Cu²+ oxid? 6.00V = Ex₁ +0.799 V 0.799 volts The student adds 6 M NH3 to the CuSO4 solution in this second cell until the Cu²+ ion is essentially all converted to Cu(NH3)42+ ion. The voltage of the cell, Ecell, goes up to 0.917 V and the Cu electrode is still negative. Find the residual concentration of Cu²+ ion in the cell. (Use Eq. 4.)

2. In another cell, the potential of the copper metal, copper(II) ion electrode was found to be 0.442 V rela- tive to a silver metal, silver ion electrode, with the copper electrode being negative. Ag+, Ag a. If the potential of the silver, silver ion electrode, E is taken to be 0.000 V in oxidation or reduction, what is the value of the potential for the oxidation reaction, EC.Cu²+oxid? Ecell = Eoxid + Ered 0.00V=[ord #-0.442 Eoxid = 0.442 6,442 volts b. If E Ag.Ag red. equals +0.799V, as in standard tables of electrode potentials, what is the value of the potential of the oxidation reaction of copper, Ecu,Cu²+ oxid? 6.00V = Ex₁ +0.799 V 0.799 volts The student adds 6 M NH3 to the CuSO4 solution in this second cell until the Cu²+ ion is essentially all converted to Cu(NH3)42+ ion. The voltage of the cell, Ecell, goes up to 0.917 V and the Cu electrode is still negative. Find the residual concentration of Cu²+ ion in the cell. (Use Eq. 4.)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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2n(s) + Cu(May) 2. In another cell, the potential of the copper metal, copper(II) ion electrode was found to be 0.442 V rela- tive to a silver metal, silver ion electrode, with the copper electrode being negative. 2n (aq) си Ag+, Ag a. If the potential of the silver, silver ion electrode, E is taken to be 0.000 V in oxidation or reduction, what is the value of the potential for the oxidation reaction, Eu.Cu²+oxid? Excell Exid + Ered. = 0.00V = [ord #-0.442 Foxid = 0.442 6,442 volts b. If E equals +0.799V, as in standard tables of electrode potentials, what is the value of the potential of the oxidation reaction of copper, Eu.Cu²+oxid? Ag.Ag red. 6.00V = Ex₁ +0.7991 0,799 volts The student adds 6 M NH3 to the CuSO4 solution in this second cell until the Cu²+ ion is essentially all converted to Cu(NH3)42+ ion. The voltage of the cell, Ecell, goes up to 0.917 V and the Cu electrode is still negative. Find the residual concentration of Cu²+ ion in the cell. (Use Eq. 4.) M
Transcribed Image Text:2n(s) + Cu(May) 2. In another cell, the potential of the copper metal, copper(II) ion electrode was found to be 0.442 V rela- tive to a silver metal, silver ion electrode, with the copper electrode being negative. 2n (aq) си Ag+, Ag a. If the potential of the silver, silver ion electrode, E is taken to be 0.000 V in oxidation or reduction, what is the value of the potential for the oxidation reaction, Eu.Cu²+oxid? Excell Exid + Ered. = 0.00V = [ord #-0.442 Foxid = 0.442 6,442 volts b. If E equals +0.799V, as in standard tables of electrode potentials, what is the value of the potential of the oxidation reaction of copper, Eu.Cu²+oxid? Ag.Ag red. 6.00V = Ex₁ +0.7991 0,799 volts The student adds 6 M NH3 to the CuSO4 solution in this second cell until the Cu²+ ion is essentially all converted to Cu(NH3)42+ ion. The voltage of the cell, Ecell, goes up to 0.917 V and the Cu electrode is still negative. Find the residual concentration of Cu²+ ion in the cell. (Use Eq. 4.) M
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