Calculate the cell potential for a reaction in a electrolytic
cell with the following half-reactions if: [U 3+] = 0.10 M, [MnO4 -
] = 0.20M, [Mn2+], and [H+ ] = 0.20 M
U 3+ + 3e -> U o Ecell = - 1.642 V
MnO4 - + 8H+ + 5e- -> Mn2+ + 4H2O Ecell = +1.51 V
An aqueous CdF2solution
is electrolyzed under 1 bar pressure using platinum
electrodes.
(a) Write the half-reactions predicted to occur at
the anode and cathode, based on the standard cell potentials given
below.
Standard Reduction Potentials (Volts) at 25 °C
F2(g)
+ 2 e-
--> 2
F-(aq)
2.870
O2(g) + 4
H3O+(aq) + 4 e- -->
6 H2O(l)
1.229
2 H2O(l) +
2 e- -->
H2(g) + 2 OH-(aq)
-0.828
Cd2+(aq)
+ 2 e-
--> Cd(s)
-0.403
Half-reaction at anode:
Half-reaction at cathode:
(b) What is...
Write the balanced, net-ionic equations for the cell reactions
for the following half-cell combinations at standard conditions. Be
sure to consider direction of spontaneity.
A. Cu/Cu2+, Zn/Zn2+
B. Ag/Ag+, Mg/Mg2+
C. Zn/Zn2+, Pb/Pb2+
D. Ni/Ni2+, Ag/Ag+
E. Cu/Cu2+, Mg/Mg2+
Write the Standard Cell Notation and Half Reactions of the
following voltaic cell combinations.
1. Zinc Nitrate (0.20 M) and Copper Nitrate (0.30 M); Copper –
Anode, Zinc – Cathode
2. Lead Sulfate (0.25 M) and Zinc Sulfate (0.50 M); Lead –
Cathode, Zinc – Anode
3. Copper Sulfate (0.65 M) and Lead Sulfate (0.20 M); Copper –
Anode, Zinc – Cathode
4. Silver Nitrate (0.15 M) and Lead Nitrate (0.40 M); Silver –
Anode, Lead – Cathode
5. Aluminum...
Use the following half-reactions to write three spontaneous
reactions, and calculate E cell for each reaction:
a. Au+ (aq) + e- ----> Au (s) E= 1.69
V
b. N2O (g) + 2H+ (aq) + 2 e-
----> N2 (g) + H2O (l) E= 1.77 V
c. Cr3+ (aq) + 3e- ---> Cr (s) E= -0.74
V
Write the overall reaction and the half-cell reactions of the
following cells, and clearly indicate the anode and the cathode for
each cell.
c) Pb|Pb2+(0.10 M)||Cu2+(0.10 M)|Cu
d) Pb|Pb2+(0.10 M)||Zn2+(0.10 M)|Zn
e) Zn|Zn2+(0.10 M)||Fe2+(0.10 M)|Fe
f) Pb|Pb2+(0.10 M)||Fe2+(0.10 M)|Fe
Write the cell reaction and electrode half-reactions and
calculate the standard potential of each of the following
cells:
a) Zn/ZnSO4(aq)//AgNO3(aq)/Ag
b) Pt/K3[Fe(CN)6](aq),
K4[Fe(CN)6](aq)//CrCl3 (aq)/Cr
Please show all steps and clear writing.
Thanks
A concentration cell is built based on the following half
reactions by using two pieces of gold as electrodes, two Au3+
solutions, 0.101 M and 0.423 M, and all other materials needed for
a galvanic cell. What will the potential of this cell be when the
cathode concentration of Au3+ has changed by 0.035 M at 307 K?
Au3+ + 3 e- → Au Eo = 1.50 V
A concentration cell is built based on the following half
reactions by using two pieces of copper as electrodes, two Cu2+
solutions, 0.145 M and 0.405 M, and all other materials needed for
a galvanic cell. What will the potential of this cell be when the
cathode concentration of Cu2+ has changed by 0.031 M at 279 K? Cu2+
+ 2 e- → Cu Eo = 0.341 V
Use the following pair of reduction half-reactions to design a
galvanic cell. Then write in the proper coefficient for each of the
species involved in the overall reaction. Water molecules and
protons are not shown in the half-reactions, but may be needed in
the overall reaction.
MnO4- (aq) ? MnO2 (s) ?o = 0.59 V NO3- (aq) ? NO (g) ?o = 0.96
V
NO3- (aq)
MnO4- (aq)
NO (g)
MnO2 (s)
H+ (aq)
H2O (l)