How many moles of electrons are transferred overall? 2. If E°cell = +1.76 V and Ecell = +1.25 V and [VO²⁺], [VO₂⁺] and [Zn²⁺] are all 1.0 M, what is the pH of the reaction? 4.31 0.69 1.70 3.61 None of the given.
How many moles of electrons are transferred overall? 2. If E°cell = +1.76 V and Ecell = +1.25 V and [VO²⁺], [VO₂⁺] and [Zn²⁺] are all 1.0 M, what is the pH of the reaction? 4.31 0.69 1.70 3.61 None of the given.
General Chemistry - Standalone book (MindTap Course List)
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter19: Electrochemistry
Section: Chapter Questions
Problem 19.70QP: Calculate the standard cell potential of the following cell at 25C. Sn(s)Sn2+(aq)I2(aq)I(aq)
Related questions
Question
1. How many moles of electrons are transferred overall?
2. If E°cell = +1.76 V and Ecell = +1.25 V and [VO²⁺], [VO₂⁺] and [Zn²⁺] are all 1.0 M, what is the pH of the reaction?
4.31
0.69
1.70
3.61
None of the given.
None of the given.
Transcribed Image Text:Increasing strength as oxidizing agent
Table of Standard Reduction Potentials
Half-Reaction
F₂(g) + 2e →→→ 2F¯ (aq)
O3(g) + 2H¹ (aq) + 2e¯ → O₂(g) + H₂O
Co³+ (aq) + e → Co (aq)
H₂O₂(aq) + 2H(aq) + 2e
→ 2H₂O
PbO₂ (s) + 4H+ (aq) + SO²(aq)
Ce+ (aq) + e
Ce³+ (aq)
+ 2e¯ →→→ PbSO4(s) + 2H₂O
2+
→Mn²+ (aq) + 4H₂O
MnO4 (aq) + 8H+ (aq) + 5e7
Au³+
(aq) + 3e - Au(s)
Cl₂(g) + 2e →→→ 2Cl¯¯(aq)
3+
Cr₂O² (aq) + 14H*(aq) + 6e¯
2Cr³+ (aq) + 7H₂O
2+
MnO₂ (s) + 4H+ (aq) + 2e7
→→Mn²+
(aq) + 2H₂O
O₂(g) + 4H+ (aq) + 4e¯ →→→ 2H₂O
Br₂() +2e7 →→→→2Br (aq)
NO3(aq) + 4H+ (aq) + 3e¯→→→→→ NO(g) + 2H₂O
2Hg²+ (aq) + 2e
Hg2+ (aq)
Hg2+ (aq) + 2e
→ 2Hg(1)
Ag+ (aq) + e →
Ag(s)
Fe³+ (aq) + e→→→→→ Fe²+ (aq)
O₂(g) + 2H+ (aq) + 2e7 →→→→H₂O₂(aq)
MnO4 (aq) + 2H₂O + 3e7
1₂(s) + 2e
21 (aq)
O₂(g) + 2H₂O + 4e¯
→→→40H(aq)
Cu(s)
Cu²+ (aq) + 2e
AgCl(s) + e
Ag(s) + Cl(aq)
SO (aq) + 4H+ (aq) + 2e¯
Cu²+ (aq) + e
Cu (aq)
Sn4+
(aq) + 2e
2H(aq) + 2e
Pb²+ (aq) + 2e-
Sn²+ (aq) + 2e
Ni²+ (aq) + 2e
Co²+
(aq) + 2e
PbSO4(s) + 2e
Cd²+ (aq) + 2e
Fe²+ (aq) + 2e
Cr³+ (aq) + 3e
Zn²+ (aq) + 2e
2H₂O + 2e
Mn²+ (aq) + 2e
A1³+ (aq) + 3e¯
Be²+ (aq) + 2e
Mg2+ (aq) + 2e
Na (aq) + e
2+
Ca²+ (aq) + 2e
Sr²+ (aq) + 2e
Ba²+ (aq) + 2e
K+ (aq) + e → K(s)
Li (aq) + e →
Li(s)
Sn²+ (aq)
H₂(g)
Pb(s)
Sn(s)
Ni(s)
Co(s)
→ Pb(s) + SO² (aq)
Cd(s)
Fe(s)
Cr(s)
Zn(s)
H₂(g) + 2OH(aq)
→→ Mn(s)
Al(s)
Be(s)
Mg(s)
Na(s)
MnO₂ (s) + 40H(aq)
SO₂(g) + 2H₂O
Ca(s)
Sr(s)
→Ba(s)
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
Transcribed Image Text:For the cell reaction
2V0₂* (aq)
+ Zn(s) + 4H* (aq) → 2VO²+ (aq) + Zn²+ (aq) + 2H₂O(1)
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