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Standard XII
Chemistry
Question
The value of
Δ
S
⊖
for the fuel cell reaction at 298 K is:
2
H
2
+
O
2
→
2
H
2
O
E
⊖
c
e
l
l
=
1.23
V
Δ
f
H
⊖
(
H
2
O
)
=
−
285.8
K
j
m
o
l
−
1
−
324.9
J
K
−
1
−
214.9
J
K
−
1
−
154.9
J
K
−
1
N
o
n
e
o
f
t
h
e
s
e
A
−
154.9
J
K
−
1
B
N
o
n
e
o
f
t
h
e
s
e
C
−
324.9
J
K
−
1
D
−
214.9
J
K
−
1
Open in App
Solution
Verified by Toppr
2
H
2
O
+
O
2
→
2
H
2
O
,
E
⊖
c
e
l
l
=
1.23
V
,
Δ
f
H
⊖
(
H
2
O
)
=
−
285.8
k
J
m
o
l
−
1
Anode :
H
2
→
2
H
⊕
+
2
e
−
Cathode :
O
2
+
4
H
⊕
+
4
e
−
→
2
H
2
O
Number of electrons transferred = 4
⇒
G
⊖
=
−
4
×
96500
×
(
+
1.23
)
=
−
474.78
k
J
Δ
G
⊖
=
Δ
H
⊖
−
T
Δ
S
⊖
⇒
Δ
S
⊖
2
×
(
−
285.8
)
−
(
−
474.78
)
298
k
J
K
−
1
=
−
324.9
J
K
−
1
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Similar Questions
Q1
The value of
Δ
S
⊖
for the fuel cell reaction at 298 K is:
2
H
2
+
O
2
→
2
H
2
O
E
⊖
c
e
l
l
=
1.23
V
Δ
f
H
⊖
(
H
2
O
)
=
−
285.8
K
j
m
o
l
−
1
View Solution
Q2
In H
2
- O
2
fuel cell the reaction occuring at cathode is :