Calculate the Eo and the E for this cell. (continued)Half ReactionAu³+ + 3e- →Cl₂(g) + 2e- →Cr₂O + 14H+ + 6e- →2Cr³+ + 7H₂OMnO₂ (s) + 4H+ + 2e → Mn²+ + 2H₂O2H₂OO₂(g) + 4H+ + 4e-Br₂(l) +2e2Br-NO + 4H+ + 3e-→ NO(g) + 2H₂O► Au(s)2C1-2+2Hg2+ + 2e → HgitHg+2e → 2Hg(l)Ag+ e-→ Ag(s)Fe³+ + e-Fe²+O₂(g) + 2H+ + 2e- → H₂O₂MnO + 2H₂O + 3e- → MnO₂ (s) + 40H-2₂(s) + 2e- →O₂(g) + 2H₂O + 4e-→ 40H-Cu²+ + 2e-AgCl(s) + e- →Cu²+ + e- →Sn4+ + 2e →→ Sn²+->21-Cu(s)► Ag(s) + CI-2H+ + 2e → H₂(g)Pb²+ + 2e-→ Pb(s)Sn²+ + 2e- 1Sn(s)Ni2+ + 2e → Ni(s)Co2+ +2eCo(s)Cd²+ + 2e → → Cd(s)Fe²+ + 2e- Fe(s)->>Cu+Cr³+ + 3eCr(s)Zn²+ + 2e → Zn(s)->2H₂O +2eH₂(g) + 2OH-Mn²+ + 2e- Mn(s)Al³+ +3e Al(s)Na+ + e- Na(s)-Ca²+ + 2e → Ca(s)Ba²+ + 2e Ba(s)K++ e->Li++eK(s)Li(s)E° (V)+1.50+1.36+1.33+1.23+1.23+1.07+0.96+0.92+0.85+0.80+0.77+0.68+0.59+0.53+0.40+0.34+0.22+0.15+0.130.00-0.13-0.14-0.25-0.28-0.40-0.44-0.74-0.76-0.83-1.18-1.66-2.71-2.87-2.90-2.93-3.05TABIAT Note: All species in aqueous solution (aq) unless otherwiseindicated. All dissolved species = 1 M; all gases = 1 atm. CuelectrodeleadCopperelectrodeCuSO4solution(a)Metercommonlead[Cu²+] = 0.0200 MVoltmeter0.412 VComVery high resistanceSalt bridgeSaturated KCl solutionMeterpositivelead[Ag+] = 0.0200 MAgelectrodeleadSilverelectrodeAgNO3solution

In an electrochemical cell, oxidation takes place at the anode and reduction takes place at the…

Answered: Calculate the Eo and the E for this…

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Chemistry

Calculate the Eo and the E for this cell.

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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Question

100%

Calculate the Eo and the E for this cell.

(continued)
Half Reaction
Au³+ + 3e- →
Cl₂(g) + 2e- →
Cr₂O + 14H+ + 6e- →2Cr³+ + 7H₂O
MnO₂ (s) + 4H+ + 2e → Mn²+ + 2H₂O
2H₂O
O₂(g) + 4H+ + 4e-
Br₂(l) +2e2Br-
NO + 4H+ + 3e-→ NO(g) + 2H₂O
► Au(s)
2C1-
2+
2Hg2+ + 2e → Hgit
Hg+2e → 2Hg(l)
Ag+ e-→ Ag(s)
Fe³+ + e-
Fe²+
O₂(g) + 2H+ + 2e- → H₂O₂
MnO + 2H₂O + 3e- → MnO₂ (s) + 40H-
2₂(s) + 2e- →
O₂(g) + 2H₂O + 4e-→ 40H-
Cu²+ + 2e-
AgCl(s) + e- →
Cu²+ + e- →
Sn4+ + 2e →→ Sn²+
->
21-
Cu(s)
► Ag(s) + CI-
2H+ + 2e → H₂(g)
Pb²+ + 2e-→ Pb(s)
Sn²+ + 2e- 1
Sn(s)
Ni2+ + 2e → Ni(s)
Co2+ +2e
Co(s)
Cd²+ + 2e → → Cd(s)
Fe²+ + 2e- Fe(s)
->>
Cu+
Cr³+ + 3e
Cr(s)
Zn²+ + 2e → Zn(s)
->
2H₂O +2eH₂(g) + 2OH-
Mn²+ + 2e- Mn(s)
Al³+ +3e Al(s)
Na+ + e- Na(s)
-
Ca²+ + 2e → Ca(s)
Ba²+ + 2e Ba(s)
K++ e->
Li++e
K(s)
Li(s)
E° (V)
+1.50
+1.36
+1.33
+1.23
+1.23
+1.07
+0.96
+0.92
+0.85
+0.80
+0.77
+0.68
+0.59
+0.53
+0.40
+0.34
+0.22
+0.15
+0.13
0.00
-0.13
-0.14
-0.25
-0.28
-0.40
-0.44
-0.74
-0.76
-0.83
-1.18
-1.66
-2.71
-2.87
-2.90
-2.93
-3.05
TABIAT Note: All species in aqueous solution (aq) unless otherwise
indicated. All dissolved species = 1 M; all gases = 1 atm.

Cu
electrode
lead
Copper
electrode
CuSO4
solution
(a)
Meter
common
lead
[Cu²+] = 0.0200 M
Voltmeter
0.412 V
Com
Very high resistance
Salt bridge
Saturated KCl solution
Meter
positive
lead
[Ag+] = 0.0200 M
Ag
electrode
lead
Silver
electrode
AgNO3
solution

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