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Chemistry
Chemistry
Problem
The standard Gibbs energy of the given cell reaction will be
3
Fe(s)
+
2
Au
3
+
(
aq
)
→
3
Fe
2
+
(
aq
)
+
2
Au(s)
3\text{Fe(s)} + 2\text{Au}^{3+}(\text{aq}) \rightarrow 3\text{Fe}^{2+}(\text{aq}) + 2\text{Au(s)}
3
Fe(s)
+
2
Au
3
+
(
aq
)
→
3
Fe
2
+
(
aq
)
+
2
Au(s)
. (Given:
E
Au
3
+
/
Au
∘
=
1.40
V
E_{\text{Au}^{3+}/\text{Au}}^{\circ} = 1.40 \text{ V}
E
Au
3
+
/
Au
∘
=
1.40
V
and
E
Fe
2
+
/
Fe
∘
=
−
0.44
V
E_{\text{Fe}^{2+}/\text{Fe}}^{\circ} = -0.44 \text{ V}
E
Fe
2
+
/
Fe
∘
=
−
0.44
V
)
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