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
Please do #3 In the picture. I am confused if the answer is d since potassium has the lowest value of standard reduction potential and therefore it will be the strongest reducing agent. Or if it is a since K+ can’t be oxidized anymore (or can it?) and I think the reduction agent needs not be oxidized. And then so is the answer A or D? Thanks for you help.
Transcribed Image Text:TABLE 18.1 Standard Electrode Potentlals at 25 °C
Reduction Half-Reaction
F) + 2 e
E (V)
+ 2F (aq)
Stronger
oxidizing agent H202(aq) + 2 H*(aq) + 2 e
2.87
+2 H20(0
→ PBSO«(s) + 2 H20(1)
→ Mn02(s) + 2 H20()
- Mn*(aq) + 4 H20(1)
Weaker
reducing agent
PbO2(s) + 4 H*(ag) + SO,²¯(aq) + 2 e
Mn04 (aq) + 4 H*(aq) + 3 e
Mno. (aq) + 8 H*(aq) + 5 e
Au+(aq) + 3e
Pb02(s) + 4 H*(aq) + 2 e
1.78
1.69
1.68
1.51
- Au(s)
1.50
- Pb2*(aq) + 2 H20()
→ 2 cr (aq)
2 C*(aq) + 7 H2O)
2 H20(1)
Mn+(aq) + 2 H,01)
+ (aq) + 3 H20()
1.46
Cl2lg) + 2 e
Cr30, (aq) + 14 H*(aq) + 6 e
02(g) + 4 H*(aq) + 4 e
MnO2(s) + 4 H*(aq) + 2 e
10, (aq) + 6 H*(aq) + 5 e
Br() + 2 e
Vo,"(aq) + 2 H*(aq) + e
NO, (aq) + 4 H*(aq) + 3 e-
1.36
1.33
→
1.23
1.21
1.20
→
2 Br (aq)
1.09
- vo?"(aq) + H20()
NOE) + 2 H20(1)
→ CIO, (aq)
1.00
0.96
CIO2() + e
Ag"(aq) + e
Fe*(aq) + e
0.95
Ag(s)
+ Fe?*(aq)
0.80
0.77
02(g) + 2 H*(aq) + 2 e
Mno, (aq) +e
b(s) + 2 e
Cu*(aq) + e
+H2O2(aq)
0.70
→ Mn0,2 (aq)
→21 (aq)
→ Cu(s)
4 OH (aq)
+ Cu(s)
→ H2SO3(aq) + H20(1)
- Cu*(aq)
- Sn*(aq)
0.56
0.54
0.52
02g) + 2 H20(1) + 4 e
Cu*(aq) + 2 e
0.40
0.34
so, (aq) + 4 H*(aq) + 2 e
Cu2*(aq) + e
Snt(aq) + 2 e
2 H*(aq) + 2 e
Fe(aq) + 3 e
0.20
0.16
0.15
- H2g)
→ Fe(s)
→ Pb(s)
→ Sn(s)
-0.036
Pb2 (aq) + 2 e
Sn2+(aq) + 2 e
N2*(aq) + 2 e
Cd*(aq) + 2 e
Fe2+(aq) + 2 e
Cr*(aq) + e
Cr (aq) + 3 e
Zn*(aq) + 2 e
-0.13
-0.14
Ni(s)
-0.23
→ Cd(s)
-0.40
- Fe(s)
Cr2*(aq)
-0.45
-0.50
- Cr(s)
-0.73
+ Zn(s)
-0.76
+ H2g) + 2 OH (aq)
→ Mn(s)
+ Al(s)
-0.83
2 H20() + 2 e
Mn2 (aq) + 2 e
-1.18
-1.66
A*(aq) + 3 e
Mg2+(aq) + 2 e
Na (aq) + e
Ca (aq) + 2 e
Ba?+(aq) + 2 e
K*(aq) + e
oxidizing agent u*(aq) + e¯
-2.37
→ Mg(s)
→ Na(s)
-2.71
- Ca(s)
-2.76
- Ba(s)
-2.90
Stronger
reducing agent
- K(s)
-2.92
Weaker
- U(s)
-3.04
Transcribed Image Text:INCH
220
52: Moleculer
SHEET
CAPACITY
3) Which substance below is the strongest reducing agent?
(b) F2(g)
(e) H2(g)
(d) K*
(c) Cr(s)
4) Please consider the following galvanic cell setup: the cell is composed of a silver rod dipped
into a silver nitrate solution connected (via a salt bridge) to a solution of a magnesium rod dipped
(a) Mg(s)
nesium chloride solution.
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