A galvanic cell is powered by the following redox reaction: 2+ 2 MnO4(aq) + 4 H,O(1) + 3 Zn(s) 2 MnO2(s) + 8 OH (aq) + 3 Zn“(aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab.
A galvanic cell is powered by the following redox reaction: 2+ 2 MnO4(aq) + 4 H,O(1) + 3 Zn(s) 2 MnO2(s) + 8 OH (aq) + 3 Zn“(aq) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab.
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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Transcribed Image Text:A galvanic cell is powered by the following redox reaction:
2+
2 Mno,(aq) + 4 H,0(1) + 3 Zn(s) →
2 MnO,(s) + 8 OH (aq) + 3 Zn“"(aq)
Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab.
Write a balanced equation for
the half-reaction that takes
place at the cathode.
Write a balanced equation for
the half-reaction that takes
place at the anode.
Calculate the cell voltage
under standard conditions.
E° = [v
Round your answer to 2
decimal places.

Transcribed Image Text:Half-Reaction
E° (V)
2H* (aq) + 2e¯ - H2 (9)
0.000
Ag* (aq) + e¯ → Ag (s)
0.7996
2H20 (I) + 2e¯ - H2 (g) + 20OH" (aq)
-0.8277
AI3+ (aq) + 3e¯ → Al (s)
-1.676
H2O2 (aq) + 2H* (aq) + 2e¯ → 2H20 (1I)
1.776
Au+ (aq) + e¯→ Au (s)
1.692
I2 (s) + 2e¯ → 21¯ (aq)
0.5355
Au3+ (aq) + 3e¯ → Au (s)
1.498
2103- (aq) + 12H* (aq) + 10e¯ → I2 (s) + 6H2O (1)
Mg2+ (aq) + 2e - Mg (s)
1.195
Ba2+ (aq) + 2e¯ → Ba (s)
-2.912
-2.372
Br2 (1) + 2e¯ → 2B1¯ (aq)
1.066
Mn2+ (aq) + 2e" → Mn (s)
-1.185
Ca2+ (aq) + 2e¯ → Ca (s)
-2.868
Mno2 (s) + 4H+ (aq) + 2e¯ → Mn2+ (aq) + 2H20 (1)
1.224
Cl2 (g) + 2e¯ → 2C1- (aq)
1.35827
Mno4- (aq) + 8H* (aq) + 5e¯ → Mn2+ (aq) + 4H2O (1)
1.507
Co2+ (aq) + 2e¯ → Co (s)
-0.28
Mnog- (aq) + 2H20 (I) + 3e¯ → MnO2 (s) + 40H¯ (aq)
0.595
Co3+ (aq) + e¯ → Co2+ (aq)
1.92
HNO2 (aq) + H+ (aq) + e¯ → NO (g) + H2O (I)
0.983
Cr2+ (aq) + 2e¯ → Cr (s)
-0.913
N2 (g) + 4H2O (1) + 4e¯ → 40H" (aq) + N2H4 (aq)
-1.16
Cr3+ (aq) + 3e¯ → Cr (s)
-0.744
NO3- (aq) + 4H* (aq) + 3e¯ → NO (g) + 2H2O (1)
0.957
Cr3+ (aq) + e¯ → Cr2+ (aq)
-0.407
Na* (aq) + e¯ → Na (s)
-2.71
Cro42- (aq) + 4H20 (I) + 3e¯ → Cr(OH)3 (s) + 50H¯ (aq)
-0.13
Ni2+ (aq) + 2e" → Ni (s)
-0.257
Cu2+ (aq) + 2e¯ → Cu (s)
0.3419
02 (g) + 4H* (aq) + 4e¯ → 2H20 (1)
1.229
Cu2+ (aq) + e- → Cu+ (aq)
0.153
02 (g) + 2H20 (1) + 4e¯ → 40H" (aq)
0.401
Cu* (aq) + e¯ → Cu (s)
0.521
02 (g) + 2H† (aq) + 2e¯ → H2O2 (aq)
Pb2+ (aq) + 2e¯ → Pb (s)
0.695
F2 (g) + 2e¯ → 2F¯ (aq)
2.866
-0.1262
Fe2+ (aq) + 2e¯ → Fe (s)
-0.447
PBSO4 (s) + H+ (aq) + 2e¯ → Pb (s) + HSO4¯ (aq)
-0.3588
Fe3+ (aq) + e- → Fe2+ (aq)
Fe3+ (aq) + 3e¯ → Fe (s)
0.771
HSO4 (aq) + 3H+ (aq) + 2e¯ → H2SO3 (aq) + H2O (1)
0.172
-0.037
Sc3+ (aq) + 3e - Sc (s)
-2.077
Sn2+
(aq) + 2e¯ – Sn (s)
-0.1375
Sn4+ (aq) + 2e¯ →
Sn2+ (aq)
0.151
VO2+ (aq) + 2H+ (aq) + e¯ →
vo2+ (aq) + H20 (I)
0.991
Zn2+
(aq) + 2e¯ →
Zn (s)
-0.7618
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