For question number 4 part b is the anode: Mg2+(aq) or Mg (s)? And is the cathode Ag+(aq) or Ag (s)? By the way I got 3.17 V for part A if that helps. Thanks!

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...
icon
Related questions
Question
100%
For question number 4 part b is the anode: Mg2+(aq) or Mg (s)? And is the cathode Ag+(aq) or Ag (s)? By the way I got 3.17 V for part A if that helps. Thanks!
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: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
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
into a magnesium chloride solution.
(a) Calculate the standard cell potential.
(b) Define the anode and cathode.
5) A major source of sodium metal is the electrolysis of molten sodium chloride. What magnitude
of current produces 1.0 kg of sodium metal in 1 hour? (M for Na =23.0g/mol).
Transcribed Image Text: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 into a magnesium chloride solution. (a) Calculate the standard cell potential. (b) Define the anode and cathode. 5) A major source of sodium metal is the electrolysis of molten sodium chloride. What magnitude of current produces 1.0 kg of sodium metal in 1 hour? (M for Na =23.0g/mol).
Expert Solution
steps

Step by step

Solved in 2 steps

Blurred answer
Knowledge Booster
Electrochemical Cells
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY