Based on the galvanic cell formed by following cell reaction (assuming all concentrations are 1.0 M):2Cu²+ (aq) + Co(s) → 2Cu¹(aq) + Co²+ (aq)a.Write the cell diagram.b. What will be the Eᵒcell? Show solution (use provided SRP table values). Increasing strength as oxidizing agentTable of Standard Reduction PotentialsHalf-ReactionF₂(g) + 2e2F (aq)03(g) + 2H+ (aq) + 2e¯ →→ O₂(g) + H₂OCo³+ (aq) + e-Co²+ (aq)H₂O₂(aq) + 2H(aq) + 2e¯→→→→→→ 2H₂OPbO₂ (s) + 4H+ (aq) + SO (aq) + 2e+ (aq) + e Ce³+ (aq)Ce4+MnO4 (aq) + 8H*(aq) + 5e¯ →→Mn²+ (aq) + 4H₂OAu³+ (aq) + 3e →→→ Au(s)2Cr³+ (aq) + 7H₂OMn²+ (aq) + 2H₂OCl₂(g) + 2e →→→ 2Cl¯ (aq)Cr₂O (aq) + 14H+ (aq) + 6e¯MnO₂ (s) + 4H+ (aq) + 2e¯→→O₂(g) + 4H(aq) + 4e¯ →Br₂(1) + 2e2Br (aq)NO3(aq) + 4H+ (aq) + 3e2Hg²+ (aq) + 2eNO(g) + 2H₂OHg₂+ (aq)Hg2+ (aq) + 2e →→→ 2Hg(1)Ag+ (aq) + e Ag(s)Fe³+ (aq) + e→→→→→→ Fe²+ (aq)O₂(g) + 2H+ (aq) + 2e →H₂O₂(aq)MnO₂ (s) + 4OH(aq)MnO4 (aq) + 2H₂O + 3e¯1₂(s) + 2e21 (aq)O₂(g) + 2H₂O + 4e4OH(aq)Cu²+ (aq) + 2eCu(s)AgCl(s) + eAg(s) + Cl(aq)SO (aq) + 4H+ (aq) + 2e →→→ SO₂(g) + 2H₂OCu²+ (aq) + eCu* (aq)Sn4+4+ (aq) + 2e¯Sn²+ (aq)H₂(g)2H*(aq) + 2ePb²+ (aq) + 2ePb(s)2+Sn²+ (aq) + 2eSn(s)Ni(s)Ni²+ (aq) + 2eCo²+→Co(s)(aq) + 2e¯PbSO4(s) + 2ePb(s) + SO² (aq)Cd(s)Cd²+ (aq) + 2eFe²+ (aq) + 2e→Fe(s)Cr³+ (aq) + 3e→ Cr(s)Zn²+(aq) + 2e¯¯→→→→→→ Zn(s)2H₂O + 2e →→→ H₂(g) + 2OH(aq)Mn²+ (aq) + 2e→ Mn(s)Al³+ (aq) + 3eAl(s)Be(s)→ Mg(s)Be²+ (aq) + 2eMg²+ (aq) + 2eNa (aq) + eCa²+ (aq) + 2eNa(s)Ca(s)Sr2²+ (aq) + 2eSr(s)2+Ba²+ (aq) + 2e →→→ Ba(s)K+ (aq) + e → K(s)Li (aq) +eLi(s)2H₂OPbSO4(s) + 2H₂OE° (V)+2.87+2.07+1.82+1.77+1.70+1.61+1.51+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+0.20+0.15+0.130.00-0.13-0.14-0.25-0.28-0.31-0.40-0.44-0.74-0.76-0.83-1.18-1.66-1.85-2.37-2.71-2.87-2.89-2.90-2.93-3.05Increasing strength as reducing agent

In the cell diagram anode is written on the right side and the cathode is on the left side. At…

Based on the galvanic cell formed by following cell reaction (assuming all concentrations are 1.0 M): 2Cu²+ (aq) + Co(s) → 2Cu¹(aq) + Co²+ (aq) a. Write the cell diagram. b. What will be the Eᵒcell? Show solution (use provided SRP table values).

Based on the galvanic cell formed by following cell reaction (assuming all concentrations are 1.0 M): 2Cu²+ (aq) + Co(s) → 2Cu¹(aq) + Co²+ (aq) a. Write the cell diagram. b. What will be the Eᵒcell? Show solution (use provided SRP table values).

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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Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

Based on the galvanic cell formed by following cell reaction (assuming all concentrations are 1.0 M):
2Cu²+ (aq) + Co(s) → 2Cu¹(aq) + Co²+ (aq)
a.
Write the cell diagram.
b. What will be the Eᵒcell? Show solution (use provided SRP table values).

Increasing strength as oxidizing agent
Table of Standard Reduction Potentials
Half-Reaction
F₂(g) + 2e2F (aq)
03(g) + 2H+ (aq) + 2e¯ →→ O₂(g) + H₂O
Co³+ (aq) + e-
Co²+ (aq)
H₂O₂(aq) + 2H(aq) + 2e¯→→→→→→ 2H₂O
PbO₂ (s) + 4H+ (aq) + SO (aq) + 2e
+ (aq) + e Ce³+ (aq)
Ce4+
MnO4 (aq) + 8H*(aq) + 5e¯ →→Mn²+ (aq) + 4H₂O
Au³+ (aq) + 3e →→→ Au(s)
2Cr³+ (aq) + 7H₂O
Mn²+ (aq) + 2H₂O
Cl₂(g) + 2e →→→ 2Cl¯ (aq)
Cr₂O (aq) + 14H+ (aq) + 6e¯
MnO₂ (s) + 4H+ (aq) + 2e¯→→
O₂(g) + 4H(aq) + 4e¯ →
Br₂(1) + 2e2Br (aq)
NO3(aq) + 4H+ (aq) + 3e
2Hg²+ (aq) + 2e
NO(g) + 2H₂O
Hg₂+ (aq)
Hg2+ (aq) + 2e →→→ 2Hg(1)
Ag+ (aq) + e Ag(s)
Fe³+ (aq) + e→→→→→→ Fe²+ (aq)
O₂(g) + 2H+ (aq) + 2e →
H₂O₂(aq)
MnO₂ (s) + 4OH(aq)
MnO4 (aq) + 2H₂O + 3e¯
1₂(s) + 2e21 (aq)
O₂(g) + 2H₂O + 4e4OH(aq)
Cu²+ (aq) + 2e
Cu(s)
AgCl(s) + e
Ag(s) + Cl(aq)
SO (aq) + 4H+ (aq) + 2e →→→ SO₂(g) + 2H₂O
Cu²+ (aq) + e
Cu* (aq)
Sn4+
4+ (aq) + 2e¯
Sn²+ (aq)
H₂(g)
2H*(aq) + 2e
Pb²+ (aq) + 2e
Pb(s)
2+
Sn²+ (aq) + 2e
Sn(s)
Ni(s)
Ni²+ (aq) + 2e
Co²+
→Co(s)
(aq) + 2e¯
PbSO4(s) + 2e
Pb(s) + SO² (aq)
Cd(s)
Cd²+ (aq) + 2e
Fe²+ (aq) + 2e
→Fe(s)
Cr³+ (aq) + 3e
→ Cr(s)
Zn²+
(aq) + 2e¯¯→→→→→→ Zn(s)
2H₂O + 2e →→→ H₂(g) + 2OH(aq)
Mn²+ (aq) + 2e
→ Mn(s)
Al³+ (aq) + 3e
Al(s)
Be(s)
→ Mg(s)
Be²+ (aq) + 2e
Mg²+ (aq) + 2e
Na (aq) + e
Ca²+ (aq) + 2e
Na(s)
Ca(s)
Sr2²+ (aq) + 2e
Sr(s)
2+
Ba²+ (aq) + 2e →→→ Ba(s)
K+ (aq) + e → K(s)
Li (aq) +eLi(s)
2H₂O
PbSO4(s) + 2H₂O
E° (V)
+2.87
+2.07
+1.82
+1.77
+1.70
+1.61
+1.51
+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
+0.20
+0.15
+0.13
0.00
-0.13
-0.14
-0.25
-0.28
-0.31
-0.40
-0.44
-0.74
-0.76
-0.83
-1.18
-1.66
-1.85
-2.37
-2.71
-2.87
-2.89
-2.90
-2.93
-3.05
Increasing strength as reducing agent

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