Balance the following skeleton reaction, calculate E cell and state whether the reaction is spontaneous: Mn²*(aq) + Co**(aq) → MnO,(8) + Co²*(aq) [acidic] Balanced reaction, including state symbols: E cell V This reaction is spontaneous. This reaction is nonspontaneous. Standard Electrode (Half-Cell) Potentials at 298 K Со (ад) + е — MnO2(s) + 4H*(aq) + 2e¯ → MnO, (aq) + 2H,0() + Зе — Со"(аq) + 2е Со(s) 2MN²*(aq) + 2e→ Mn(s) Co2*(aq) Mn²*(aq) + 2H2O(1) MnO2(s) + 40H (aq) E° = 1.82 V E° = 1.23 V E° = 0.59 V E° = -0.28 V E° =-1.18 V
Balance the following skeleton reaction, calculate E cell and state whether the reaction is spontaneous: Mn²*(aq) + Co**(aq) → MnO,(8) + Co²*(aq) [acidic] Balanced reaction, including state symbols: E cell V This reaction is spontaneous. This reaction is nonspontaneous. Standard Electrode (Half-Cell) Potentials at 298 K Со (ад) + е — MnO2(s) + 4H*(aq) + 2e¯ → MnO, (aq) + 2H,0() + Зе — Со"(аq) + 2е Со(s) 2MN²*(aq) + 2e→ Mn(s) Co2*(aq) Mn²*(aq) + 2H2O(1) MnO2(s) + 40H (aq) E° = 1.82 V E° = 1.23 V E° = 0.59 V E° = -0.28 V E° =-1.18 V
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.44QE: For each of the reactions, calculate E from the table of standard potentials, and state whether the...
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Balance the following skeleton reaction, calculate Eo cell, and state whether the reaction is spontaneous:
Mn2+(aq) + Co3+(aq) → MnO2(s) + Co2+(aq) [acidic]
Balanced reaction, including state symbols:
Transcribed Image Text:Here's a hint!
Look up the value for E
for each substance.
half-cell
![Balance the following skeleton reaction, calculate E
and state whether the reaction is spontaneous:
cell
Mn2*(aq) + Co**(aq)
MnO2(s) +
Co2*(aq)
[acidic]
Balanced reaction, including state symbols:
E
cell
V
This reaction is spontaneous.
This reaction is nonspontaneous.
Standard Electrode (Half-Cell) Potentials at 298 K
Со (ад) + е — Соt (ag)
E° = 1.82 V
MnO2(s) + 4H*(aq) + 2e¯ →
Mn2*(aq) + 2H2O(1)
E° = 1.23 V
MnO4 (аq) + 2H,0() + Зе —
Co²*(aq)
2Mn2*(aq) + 2e¯
MnO2(s) + 40H (aq)
E° = 0.59 V
+ 2e → Co(s)
E° = -0.28 V
→ Mn(s)
E° = -1.18 V](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F71d7a67c-bd18-4e8c-9024-55cc75fdbac3%2F378ec0c0-d888-42db-8676-b2b0aad2843f%2Fs80ygy_processed.png&w=3840&q=75)
Transcribed Image Text:Balance the following skeleton reaction, calculate E
and state whether the reaction is spontaneous:
cell
Mn2*(aq) + Co**(aq)
MnO2(s) +
Co2*(aq)
[acidic]
Balanced reaction, including state symbols:
E
cell
V
This reaction is spontaneous.
This reaction is nonspontaneous.
Standard Electrode (Half-Cell) Potentials at 298 K
Со (ад) + е — Соt (ag)
E° = 1.82 V
MnO2(s) + 4H*(aq) + 2e¯ →
Mn2*(aq) + 2H2O(1)
E° = 1.23 V
MnO4 (аq) + 2H,0() + Зе —
Co²*(aq)
2Mn2*(aq) + 2e¯
MnO2(s) + 40H (aq)
E° = 0.59 V
+ 2e → Co(s)
E° = -0.28 V
→ Mn(s)
E° = -1.18 V
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