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Chemistry
Chemistry
Problem
Consider the following cell reaction :
2
Fe
(
s
)
+
O
2
(
g
)
+
4
H
+
⟶
2
Fe
2
+
(
aq
)
+
2
H
2
O
(
l
)
2\text{Fe} (\text{s}) + \text{O}_2 (\text{g}) + 4\text{H}^+ \longrightarrow 2\text{Fe}^{2+} (\text{aq}) + 2\text{H}_2\text{O} (\text{l})
2
Fe
(
s
)
+
O
2
(
g
)
+
4
H
+
⟶
2
Fe
2
+
(
aq
)
+
2
H
2
O
(
l
)
E
∘
=
1.67
V
E^{\circ} = 1.67 \text{ V}
E
∘
=
1.67
V
[
Fe
2
+
]
=
10
−
3
M
[\text{Fe}^{2+}] = 10^{-3} \text{ M}
[
Fe
2
+
]
=
1
0
−
3
M
,
P
(
O
2
)
=
0.1
atm
\text{P}(\text{O}_2) = 0.1 \text{ atm}
P
(
O
2
)
=
0.1
atm
and
pH
=
3
\text{pH} = 3
pH
=
3
, the cell potential at
25
∘
C
25^{\circ}\text{C}
2
5
∘
C
is : a.
1.47
V
1.47 \text{ V}
1.47
V
b.
1.77
V
1.77 \text{ V}
1.77
V
c.
1.87
V
1.87 \text{ V}
1.87
V
d.
1.57
V
1.57 \text{ V}
1.57
V
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