Chapter Chosen
Electrochemistry
Book Chosen
Chemistry I
Subject Chosen
Chemistry
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Class 10
Class 12
Electrochemistry
Calculate ΔG° for the reaction
Cu
2
+
(
aq
)
+
Fe
(
s
)
→
Fe
2
+
(
aq
)
+
Cu
(
s
)
(
Given
E
°
Cu
2
+
/
Cu
=
0
.
34
V
,
E
°
Fe
3
+
/
Fe
=
-
0
.
44
V
,
F
=
96500
e
mol
-
1
)
E
°
cell
=
E
°
cathode
-
E
°
anode
=
E
°
Cu
2
+
/
Cu
-
E
°
Fe
3
+
/
Fe
=
0
.
34
V
-
(
-
0
.
44
V
)
=
0
.
78
V
∆
r
G
=
-
nFE
°
=
-
2
×
96500
×
0
.
78
(
∵
n
=
2
)
=
-
150540
J
=
-
150
.
54
kJ
128 Views
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Calculate the equilibrium constant for the cell reaction:
4
Br
-
+
O
2
+
4
H
+
→
2
Br
2
+
2
H
2
O
(Given
E
°
cell
=
0
.
16
)
we have given that
E
0
= 0.16
log
K
C
=
nE
°
cell
0
.
0591
E
°
cell
=
0
.
16
V
,
n
=
4
log
K
C
=
(
4
)
×
(
0
.
16
V
)
(
0
.
0591
V
)
=
10
.
8
K
C
=
Antilog
10
.
8
=
6
.
31
×
10
10
181 Views
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Calculate the equilibrium constant K
c
for the reaction at 298 K.
3
Sn
4
+
+
2
Cr
⇋
3
Sn
2
+
+
2
Cr
3
+
(
Given
E
°
Sn
4
+
/
Sn
2
+
=
0
.
15
V
;
E
°
Cr
3
+
/
Cr
=
-
074
V
)
.
=
0
.
34
V
;
E
°
cell
=
E
°
Sn
4
+
/
Sn
2
+
-
E
°
Sn
4
+
/
Sn
2
+
-
E
°
Cr
3
+
/
Cr
=
0
.
15
-
(
-
0
.
74
)
=
0
.
89
V
It is clear from the given equation that electrons
involved in the reaction (n) = 6
log
K
C
=
E
°
cell
×
n
0
.
059
or
log
K
C
=
0
.
89
×
6
0
.
059
=
90
.
508
or
K
C
=
antilog
90
.
508
or
K
C
=
3
.
221
×
10
90
.
155 Views
Calculate the equilibrium constant for the reaction at 298 K
Cu
(
s
)
+
Cl
2
(
g
)
⇌
CuCl
2
(
aq
)
Given:
E
°
Cu
2
+
/
Cu
=
0
.
34
V
;
E
°
Cl
2
+
/
Cl
-
=
1
.
36
V
,
R
=
8
.
314
J
K
-
1
mol
-
1
R
=
96500
C
mol
-
1
E
°
cell
=
E
°
cathode
-
E
°
anode
=
1
.
36
-
0
.
34
=
1
.
02
V
Equilibrium constant,
log
K
C
=
E
°
cell
×
nF
2
.
303
RT
or
log
K
C
=
1
.
02
×
2
×
96500
2
.
303
×
8
.
314
×
298
=
34
.
57
or
K
C
=
Antilog
(
34
.
57
)
=
3
.
715
×
10
34
784 Views
The standard electrode potential for Daniell cell is 1.1 V. Calculate the standard Gibbs energy for the reaction:
Zn
(
s
)
+
Cu
2
+
(
aq
)
→
Zn
2
+
(
aq
)
+
Cu
(
s
)
∆
r
G
°
=
-
nFE
°
n
=
2
and
F
=
96500
C
E
°
cell
=
+
1
.
10
∆
r
G
°
=
-
2
×
96500
×
1
.
10
or
∆
r
G
°
=
-
212300
J
W
max
=
-
∆
r
G
°
=
212300
J
1162 Views
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