For the following half-reactions: Fe²+ (aq) → Fe(s) Zn²+ (aq) → Zn(s) a. What will be the overall balanced reaction if you want to make a galvanic cell? b. What is the standard cell potential, Eᵒcell? Show solution (use provided SRP table values). C. If the initial concentrations are [Fe²+]=1.0×105 M and [Zn²+]=0.10 M, what is Ecell? (Show solution)
For the following half-reactions: Fe²+ (aq) → Fe(s) Zn²+ (aq) → Zn(s) a. What will be the overall balanced reaction if you want to make a galvanic cell? b. What is the standard cell potential, Eᵒcell? Show solution (use provided SRP table values). C. If the initial concentrations are [Fe²+]=1.0×105 M and [Zn²+]=0.10 M, what is Ecell? (Show solution)
Chapter18: Introduction To Electrochemistry
Section: Chapter Questions
Problem 18.18QAP
Related questions
Question
![For the following half-reactions:
Fe²+ (aq) → Fe(s)
Zn²+ (aq) →→→ Zn(s)
-
a. What will be the overall balanced reaction if you want to make a galvanic cell?
b. What is the standard cell potential, Eᵒcell? Show solution (use provided SRP table values).
C.
If the initial concentrations are [Fe²+] =1.0×105 M and [Zn²+]=0.10 M, what is Ecell? (Show solution)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8dd5ecd4-9d74-4d0a-a174-44f6ad2c456d%2F0060b185-5ee8-481a-a02c-0b848f02219f%2Fbqv5sq_processed.png&w=3840&q=75)
Transcribed Image Text:For the following half-reactions:
Fe²+ (aq) → Fe(s)
Zn²+ (aq) →→→ Zn(s)
-
a. What will be the overall balanced reaction if you want to make a galvanic cell?
b. What is the standard cell potential, Eᵒcell? Show solution (use provided SRP table values).
C.
If the initial concentrations are [Fe²+] =1.0×105 M and [Zn²+]=0.10 M, what is Ecell? (Show solution)
Transcribed Image Text: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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