for Pd, Ti, Il (Assuming Cr₂O,(aq), H(aq) is from page 7 is known) A4/ Format Times New... ✓ BIU 12pt PRI ON 1. Cr₂0,2(aq) + 14H(aq) + 6e- 2 Cr³(aq) + 7 H₂O(1) 2.? 3.? 4. ? +1.23 V www 3
for Pd, Ti, Il (Assuming Cr₂O,(aq), H(aq) is from page 7 is known) A4/ Format Times New... ✓ BIU 12pt PRI ON 1. Cr₂0,2(aq) + 14H(aq) + 6e- 2 Cr³(aq) + 7 H₂O(1) 2.? 3.? 4. ? +1.23 V www 3
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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GENERAL CHEMISTRY
UPVOTE WILL BE GIVEN. PLEASE WRITE THE COMPLETE SOLUTIONS. FOLLOW THE INSTRUCTIONS. BOX THE FINAL ANSWERS.
Transcribed Image Text:DEVELOPING a REDOX TABLE
We can use standard cells and their measured cell potentials to develop a redox table.
PURPOSE: The purpose of this exercise is to use the concepts and the rules of the standard cells to
develop a redox table.
PROBLEM: What is the table of relative strengths of oxidizing and reducing agents based on measured
cell potentials? (You are making a MINI Table of Redox based on cell potentials from the evidence
below)
DESIGN: Several Cells are investigated; each cell has at least one half-cell in common with one of the
other cells. The cell potentials are measured, and the positive and negative electrodes of each cell are
identified.
EVIDENCE:
Negative Electrode (-)
Pd(s) Pd² (aq) || Cr₂O²(aq), H(aq) | C(s)
Ti(s) Ti²(aq)
TI" (aq) | Tl(s)
TI(s) | TI" (aq) || Pd²(aq) | Pd(s)
ANALYSIS: (Mini TABLE of Redox, including Reduction half reaction with Reduction Potentials
for Pd, Ti, Tl (Assuming Cr₂O₂(aq), H(aq) is from page 7 is known)
Format
Times New... ✓
Positive Electrode (+)
BI
12pt
U
v
A
7
9
=&C
1. Cr₂0-²(aq) + 14H(aq) + 6e- 2 Cr³+ (aq) + 7 H₂O(1)
2.?
3. ?
4. ?
E cell net +0.35 V
E cell net +1.29 V
Ecell net +1.32 V
+ v
+1.23 V
www
3
Table of Selected Standard Electrode Potentials*
Reduction Half-Reaction
F₂(g) + 2e at 2F (aq)..
PbO₂(s) + SO³(aq) + 4H(aq) + 2e PbSO,09 + 2H₂O(1)
MnO, (aq) + 8H(aq) + Se
Mn(aq) + 4H₂O(1)
Au (aq) + 3e
3e Au(s)
at
CIO, (aq) + SH'(aq) + 8e
Seat CT (aq) + 4H₂O(1)
Cl₂(g) 2 e
2 et 2CT (aq)
2 HNO (aq) + 4H(aq) + 4e
4e a N₂O(g) + 3H₂O(1)
Cr₂O₂ (aq) + 14 H(aq) + 6e at 2 Cr" (aq) + 7H₂O(D)
O(g) + 4H(aq) + 4 en 2H₂O(1)
MnO,(s) + 4H*(aq) + 2e
2 en Mn(aq) + 2H₂O(l)
2 Br(aq)
an Hg(1)
Bryl) 2e
Hg(aq) + 2e
2e
OCT (aq) + H₂O) 2e
2 NO, (aq) + 4H(aq) + 2e
Ag (aq) + e
Fe(aq) + e
O(g) + 2H(aq) + 2e
16) + 2 e
O(g) + 2H₂O) 4e
Cu(aq) + 2 en
So, (aq) + 4H(aq) + 2e
Sn(aq) + 2e
Cl(aq) + 2OH(aq)
N₂O₂(g) + 2H₂O(1)
Ag(s)
anFe²(aq)
H₂O₂(1)
21 (aq)
4 OH(aq)
Cu(s)
an
Page 7
S(s) + 2H(aq) + 2e a
AgBr(s) + e
H₂S(aq)
Ag(s) + Br(aq)
an H₂(g)
an Pb(s)
at Sn(s)
2 H(aq) + 2 e
Pb(aq) + 2e
Sn2(aq) + 2 e
Agl(s) + e
Ni²(aq) + 2e an
Co² (aq) + 2 en
PbSO4(s) + 2e
Se(s) + 2 H'(aq) + 2e
Cd²(aq) + 2e
Cr" (aq) + e
Fe²(aq) + 2e
an
a
H₂SO,(aq) + H₂O(1)
Sn² (aq)
Electrical Potential E° (V)
+2.87
+1.69
+1.51
+1.50
+1.39
+1.36
+1.30
+1.23
Ag(s) + 1'(aq)
Ni(s)
Co(s)
Pb(s) + SO² (aq)
H₂Selaq)
Cd(s)
Cr³(aq)
Fe(s)
NO(g) + 2OH(aq).
2 Ag(s) + S² (aq)
NO₂ (aq) + H₂O(1) +
Ag-S(s) + 2 e
Zn(aq) + 2e
2 H₂O(1) 2e"
Cr(aq) + 2 c
2 e
Se(s) 2e
2e
so (aq) + H₂O) 2e
AP (aq) + 3e
an Al(s)
Mg(aq) + 2 et Mg(s)
Na (aq) + en Na(s)
Ca(aq) + 2e at Ca(s)
Ba(aq) + 2 c n Ba(s)
e
K'(aq) + e an K(s)
Li' (aq) + canLi60.
*For 1.0 mol/L solutions at 298.15 K (25.00 "C) and a pressure of 101.325 kPa
pt Zn(s)....
at H₂(g) + 2OH(aq)
an Cr(s)
an Se (aq)
SO, (aq) + 2OH(aq)
+1.23
+1.22
+1.07
+0.85
+0.84
+0.80
+0.80
+0.77
+0.70
+0.54
+0.40
+0.34
+0.17
+0.15
+0.14
+0.07
0.00
-0.13
-0.14
-0.15
-0.26
-0.28
-0.36
-0.40
-0.40
-0.41
-0.45
-0.46
-0.69
-0.76
-0.83
-0.91
-0.92
-0.93
-1.66
-2.37
-2.71
-2.87
-2.91
-2.93
<-3.04
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