1.How does the cell you will set-up in lab differ from the typical electrochemical cell where the two half-cells are physically separate from each other? (electrolytic cell) 2. Thinking about the Nernst Equation, select a half-cell reaction in which the value of n would be 2. a) Cu2+ (aq) + 2e- → Cu0; (s) b) Cu1+ (aq) + 1e- → Cu0; (s) c) Al3+ (aq) + 3e- → Al0; (s)
1.How does the cell you will set-up in lab differ from the typical
2.
Thinking about the Nernst Equation, select a half-cell reaction in which the value of n would be 2.
a) Cu2+ (aq) + 2e- → Cu0; (s)
b) Cu1+ (aq) + 1e- → Cu0; (s)
c) Al3+ (aq) + 3e- → Al0; (s)
d) Pu3+ (aq) + 1e- → Pu2+ (aq)
3.
In a half-reaction with the following equation:
MnO2 (s) + 4 H+ + 2 e- → Mn2+ + 2 H2O
E° = 1.23
The oxidation state of Mn in MnO2 is=?
4.
In a half-reaction with the following equation:
MnO2 (s) + 4 H+ + 2 e- → Mn2+ + 2 H2O
E° = 1.23
Mn is?
5.
Using the half-reaction given in Question #3, determine the reduction potential if the cell is composed of:
[Mn2+] = 4.3 x 10-4 M
pH = 2.45
a) 1.23 V
b) 1.02 V
c) 0.0296 V
d) 3.55 x 10-3 V
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