Standard Reduction Potentials (25°C) Half-Cell Reactions Eº F2(g) + 2e-1 -> 2F-1 (aq) +2.87 Oxp +2H+1 +21 (aq) O2(g) + H2O(l) +2.08 S208² (aq) + 2e-1 ---------> 2 SO4²* (aq) +2.05 Co³+ (aq) +e-1 Co (aq) +1.82 H₂O2(aq) +2 H+1 (aq) MnO4 (aq) -1 +4 H+1 +3e-1 PbO2(s) + SO4(aq) +4 H+1 2 HOCK +2 H+1 (aq) (aq) + 2e-1. 2 H₂O(1) +1.77 > MnO2(s) + 2 H₂O (1) +1.695 + 2e-1 PbSO4(s) + 2 H2O(1) +1.69 (aq) + 2e-1 Cl2(g) + 2 H2O(1) +1.63 Mp3+ + e-1 (aq) ---------> Mn (aq) +1.51 MnO4 (aq) -1 +8H+1 PbO2(s)+4 H+1 +50-1 (aq) Mn2+(aq) +4 H₂O (1) +1.49 (aq) +21 -> Pb²+ (aq) +2 H₂OD +1.46 BrO3(aq) +6 H+ (aq) +60-1 (aq) --> Br-1 +3 H₂O(1) +1.44 (aq) Au+ +3e-1 Au(s) +1.42 Cl) + 2e-1 > 2 CI-¹ (aq) +1.36 Cr₂0) +14 H+1 +60-1 (aq) ·2C³ (aq) +7 HO +1.33 O3(g) + H2O(l) + 2e-1 ---------> O2(g) + 2 OH¹ (aq) +1.24 MnO2(s) +4 H+1 +2e-1 ---------> Mn2+ (aq) (aq) + 2 HyOn +2 H₂O(1) +1.23 02(g) + 4 H+1 +4e-1 (aq) 2 H₂O(1) +1.23 Pt+ (aq) +2e-1 ·Pl(s) +1.20 (aq) +3 H+1 +2e-1 +1 (aq) Br2(aq) NO3 NO +2e-1 (aq) 2 Hg2+(aq) HO₂(aq) + H₂O+2e1. 2 NO3(aq) + 4 H+1 Ag +e-1 ---------> Ag(s) 2 Br¹ (aq) +1.07 +4 H+1 (aq) +3e-1 ---------> NO(g) + 2 H₂O(1) +0.96 +2e-1 (aq) HNO2(g) + H2O(1) +0.94 Hg₂2+ (aq) +0.91 ----------> 3 OH-1 (aq) +0.87 +2e-1 (aq) 2 NO2(g) + 2H2O(1) +0.80 +0.80 Fe +e-1 (aq) -> Fe²+ (aq) +0.77 Ozig) +2H+1 +2e-1 (aq) H₂O) +0.69 12(s) + 2e-1 ----------> 2 1-¹ (aq) +0.54 NiO2()+2 H₂O)+2e-1 ----------> Ni(OH)2+2 OH¹ (aq) +0.49 Using the following standard reduction potential table. Select 8 sets of metal atoms (4 pairs) from the table and determine the redox reaction that would occur between each pair. For example, you may choose platinum (Pt) and gold (Au). Using the table, you would identify that Au3+ will oxidize Pt, resulting in this overall reaction: 2Au+3Pt(s) 3Pt2)+2Au(s) (aq) (aq) Using your 4 pairs, determine the resulting redox reactions. Make sure the reactions are balanced for atoms and electron transfer!
Standard Reduction Potentials (25°C) Half-Cell Reactions Eº F2(g) + 2e-1 -> 2F-1 (aq) +2.87 Oxp +2H+1 +21 (aq) O2(g) + H2O(l) +2.08 S208² (aq) + 2e-1 ---------> 2 SO4²* (aq) +2.05 Co³+ (aq) +e-1 Co (aq) +1.82 H₂O2(aq) +2 H+1 (aq) MnO4 (aq) -1 +4 H+1 +3e-1 PbO2(s) + SO4(aq) +4 H+1 2 HOCK +2 H+1 (aq) (aq) + 2e-1. 2 H₂O(1) +1.77 > MnO2(s) + 2 H₂O (1) +1.695 + 2e-1 PbSO4(s) + 2 H2O(1) +1.69 (aq) + 2e-1 Cl2(g) + 2 H2O(1) +1.63 Mp3+ + e-1 (aq) ---------> Mn (aq) +1.51 MnO4 (aq) -1 +8H+1 PbO2(s)+4 H+1 +50-1 (aq) Mn2+(aq) +4 H₂O (1) +1.49 (aq) +21 -> Pb²+ (aq) +2 H₂OD +1.46 BrO3(aq) +6 H+ (aq) +60-1 (aq) --> Br-1 +3 H₂O(1) +1.44 (aq) Au+ +3e-1 Au(s) +1.42 Cl) + 2e-1 > 2 CI-¹ (aq) +1.36 Cr₂0) +14 H+1 +60-1 (aq) ·2C³ (aq) +7 HO +1.33 O3(g) + H2O(l) + 2e-1 ---------> O2(g) + 2 OH¹ (aq) +1.24 MnO2(s) +4 H+1 +2e-1 ---------> Mn2+ (aq) (aq) + 2 HyOn +2 H₂O(1) +1.23 02(g) + 4 H+1 +4e-1 (aq) 2 H₂O(1) +1.23 Pt+ (aq) +2e-1 ·Pl(s) +1.20 (aq) +3 H+1 +2e-1 +1 (aq) Br2(aq) NO3 NO +2e-1 (aq) 2 Hg2+(aq) HO₂(aq) + H₂O+2e1. 2 NO3(aq) + 4 H+1 Ag +e-1 ---------> Ag(s) 2 Br¹ (aq) +1.07 +4 H+1 (aq) +3e-1 ---------> NO(g) + 2 H₂O(1) +0.96 +2e-1 (aq) HNO2(g) + H2O(1) +0.94 Hg₂2+ (aq) +0.91 ----------> 3 OH-1 (aq) +0.87 +2e-1 (aq) 2 NO2(g) + 2H2O(1) +0.80 +0.80 Fe +e-1 (aq) -> Fe²+ (aq) +0.77 Ozig) +2H+1 +2e-1 (aq) H₂O) +0.69 12(s) + 2e-1 ----------> 2 1-¹ (aq) +0.54 NiO2()+2 H₂O)+2e-1 ----------> Ni(OH)2+2 OH¹ (aq) +0.49 Using the following standard reduction potential table. Select 8 sets of metal atoms (4 pairs) from the table and determine the redox reaction that would occur between each pair. For example, you may choose platinum (Pt) and gold (Au). Using the table, you would identify that Au3+ will oxidize Pt, resulting in this overall reaction: 2Au+3Pt(s) 3Pt2)+2Au(s) (aq) (aq) Using your 4 pairs, determine the resulting redox reactions. Make sure the reactions are balanced for atoms and electron transfer!
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
question 1 ) loook at the pictures
question 2)
Draw the four voltaic cells from Lesson that you picked using only metals, indicating the following:
- Anode and cathode
- Flow of electrons
- Short-form notation
- Cell potential
Transcribed Image Text:Standard Reduction Potentials (25°C)
Half-Cell Reactions
Eº
F2(g) + 2e-1
-> 2F-1
(aq)
+2.87
Oxp
+2H+1 +21
(aq)
O2(g) + H2O(l)
+2.08
S208² (aq) + 2e-1
---------> 2 SO4²* (aq)
+2.05
Co³+
(aq)
+e-1
Co (aq)
+1.82
H₂O2(aq) +2 H+1
(aq)
MnO4 (aq)
-1 +4 H+1 +3e-1
PbO2(s) + SO4(aq) +4 H+1
2 HOCK +2 H+1
(aq)
(aq) + 2e-1.
2 H₂O(1)
+1.77
> MnO2(s) + 2 H₂O (1)
+1.695
+ 2e-1
PbSO4(s) + 2 H2O(1)
+1.69
(aq) + 2e-1
Cl2(g) + 2 H2O(1)
+1.63
Mp3+ + e-1
(aq)
---------> Mn (aq)
+1.51
MnO4 (aq)
-1 +8H+1
PbO2(s)+4 H+1
+50-1
(aq)
Mn2+(aq)
+4 H₂O (1)
+1.49
(aq)
+21
-> Pb²+
(aq)
+2 H₂OD
+1.46
BrO3(aq) +6 H+
(aq)
+60-1
(aq)
--> Br-1 +3 H₂O(1)
+1.44
(aq)
Au+ +3e-1
Au(s)
+1.42
Cl)
+ 2e-1
> 2 CI-¹
(aq)
+1.36
Cr₂0)
+14 H+1 +60-1
(aq)
·2C³
(aq)
+7 HO
+1.33
O3(g) + H2O(l) + 2e-1
--------->
O2(g) + 2 OH¹ (aq)
+1.24
MnO2(s)
+4 H+1 +2e-1 ---------> Mn2+
(aq)
(aq) + 2 HyOn
+2 H₂O(1)
+1.23
02(g) + 4 H+1
+4e-1
(aq)
2 H₂O(1)
+1.23
Pt+ (aq)
+2e-1
·Pl(s)
+1.20
(aq)
+3 H+1
+2e-1
+1
(aq)
Br2(aq)
NO3
NO
+2e-1
(aq)
2 Hg2+(aq)
HO₂(aq) + H₂O+2e1.
2 NO3(aq) + 4 H+1
Ag +e-1 ---------> Ag(s)
2 Br¹ (aq)
+1.07
+4 H+1
(aq)
+3e-1
--------->
NO(g) + 2 H₂O(1)
+0.96
+2e-1
(aq)
HNO2(g) + H2O(1)
+0.94
Hg₂2+
(aq)
+0.91
----------> 3 OH-1
(aq)
+0.87
+2e-1
(aq)
2 NO2(g) + 2H2O(1)
+0.80
+0.80
Fe
+e-1
(aq)
-> Fe²+
(aq)
+0.77
Ozig)
+2H+1
+2e-1
(aq)
H₂O)
+0.69
12(s) + 2e-1
----------> 2 1-¹ (aq)
+0.54
NiO2()+2 H₂O)+2e-1
----------> Ni(OH)2+2 OH¹
(aq)
+0.49
Transcribed Image Text:Using the following standard reduction potential table. Select 8 sets
of metal atoms (4 pairs) from the table and determine the redox
reaction that would occur between each pair.
For example, you may choose platinum (Pt) and gold (Au). Using the
table, you would identify that Au3+ will oxidize Pt, resulting in this
overall reaction:
2Au+3Pt(s) 3Pt2)+2Au(s)
(aq)
(aq)
Using your 4 pairs, determine the resulting redox reactions. Make sure
the reactions are balanced for atoms and electron transfer!
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