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Galvanic Cells
Galvanic Cells
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Galvanic Cell
Example
Definitions
Formulaes
Electrode Potential
Example
Definitions
Formulaes
Measuring Electrode Potential
Example
Definitions
Formulaes
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Daniel cell
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Galvanic Cell of Copper and Silver Nitrate
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Oxidation and Reduction Potential
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Reference Electrodes
25 mins
Measurement of Standard Potential of Zinc and Copper Electrodes Using S.H.E as Reference Electrode
24 mins
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Galvanic Cell
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Cell Notation and Cell Potential of Galvanic Cell
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Electrode Potential
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Measurement of Electrode Potential
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Important Questions
Calculate the potential of hydrogen electrode in contact with a solution whose
p
H
is
1
0
.
Medium
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>
Depict the galvanic cell in which the reaction
Z
n
(
s
)
+
2
A
g
+
(
a
q
)
→
Z
n
2
+
(
a
q
)
+
2
A
g
(
s
)
takes place. Further show:
(i) Which of the electrode is negatively charged?
(ii) The carriers of the current in the cell.
(iii) Individual reaction at each electrode.
Hard
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>
Predict the products of electrolysis in each of the following:
(i) An aqueous solution of
A
g
N
O
3
with silver electrodes.
(ii) An aqueous solution of
A
g
N
O
3
with platinum electrodes.
(iii) A dilute solution of
H
2
S
O
4
with platinum electrodes.
(iv) An aqueous solution of
C
u
C
l
2
with platinum electrodes
Hard
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>
Two half-reaction of an electrochemical cell are given below :
M
n
O
4
−
(
a
q
)
+
8
H
+
+
5
e
−
→
M
n
2
+
(
a
q
)
+
4
H
2
O
(
l
)
;
E
∘
=
+
1
.
5
1
V
S
n
2
+
(
a
q
)
→
S
n
4
+
(
a
q
)
+
2
e
−
,
E
∘
=
+
0
.
1
5
V
Construct the redox equation from the standard potential of the cell and predict if the reaction is reactant favoured or product favoured .
Hard
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>
Describe the construction and working of calomel electrode.
Medium
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>
Write the cell reaction and calculate
E
o
cell of the following electrochemical cell:
(
s
)
A
l
∣
(
1
M
)
(
a
q
.
)
A
l
3
+
∣
∣
(
1
M
)
(
a
q
.
)
Z
n
2
+
∣
(
s
)
Z
n
E
A
l
o
=
−
1
.
6
6
V
E
Z
n
o
=
−
0
.
7
6
V
Hard
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>
a) Draw labelled diagram of Standard Hydrogen Electrode ( SHE ).
Write its half cell reaction of
E
o
value.
b) Calculate
△
r
G
⊝
for the following reaction :
F
e
(
a
q
)
+
2
+
A
g
(
a
q
)
+
→
F
e
(
a
q
)
+
3
+
A
g
(
s
)
.
(Given :
E
C
e
l
l
0
=
+
0
.
0
3
V
,
F
=
9
6
5
0
0
C
).
Medium
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>
A standard hydrogen electrode has a zero potential because:
Medium
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>
Calculate the electrode potential at a copper electrode dipped in a
0
.
1
M
solution of copper sulphate at
2
5
∘
C
. The standard electrode potential of
C
u
2
+
/
C
u
system is
0
.
3
4
v
o
l
t
at
2
9
8
K
.
Easy
View solution
>
Using the standard electrode potentials given in Table
3
.
1
, predict if the reaction between the following is feasible:
(i)
F
e
3
+
(
a
q
)
and
I
−
(
a
q
)
(ii)
A
g
+
(
a
q
)
and
C
u
(
s
)
(iii)
F
e
3
+
(
a
q
)
and
B
r
−
(
a
q
)
(iv)
A
g
(
s
)
and
F
e
3
+
(
a
q
)
(v)
B
r
2
(
a
q
)
and
F
e
2
+
(
a
q
)
Hard
View solution
>