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Tardigrade
Question
Chemistry
For the given cell ; Cu ( s )| Cu 2+( C 1 M ) | Cu 2+( C 2 M )| Cu ( s ) change in Gibbs energy (Δ G) is negative, if
Q. For the given cell ;
C
u
(
s
)
∣
∣
C
u
2
+
(
C
1
M
)
∥
C
u
2
+
(
C
2
M
)
∣
∣
C
u
(
s
)
change in Gibbs energy
(
Δ
G
)
is negative, if
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A
C
1
=
2
C
2
23%
B
C
2
=
C
1
/
2
18%
C
C
1
=
C
2
35%
D
C
2
=
2
C
1
23%
Solution:
Δ
G
=
−
n
F
E
cell
Δ
G
is negative, if
E
cell
is positive
Anode:
C
u
(
s
)
→
C
u
+
2
(
C
1
)
+
2
e
−
:
E
∘
Cell reaction
:
C
u
+
2
(
C
2
)
⟶
C
u
+
2
(
C
1
)
E
ce
n
∘
=
0
Cathode
:
C
u
+
2
(
C
2
)
+
2
e
−
→
C
u
(
S
)
:
−
E
∘
E
cell
=
E
ce
ll
∘
−
n
F
2.303
RT
lo
g
Q
E
cell
=
0
−
n
F
2.303
RT
lo
g
(
C
2
C
1
)
E
cell
>
0
:
if
C
2
C
1
<
1
⇒
C
1
<
C
2