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Chemistry
Chemistry
Problem
The half-reaction
F
e
2
+
(
a
q
)
→
F
e
3
+
(
a
q
)
+
e
−
\mathrm{Fe^{2+}(aq) \;\rightarrow\; Fe^{3+}(aq) + e^-}
F
e
2
+
(
aq
)
→
F
e
3
+
(
aq
)
+
e
−
describes the oxidation of iron(II) ion. How many moles of electrons are lost when
0.40
mol
0.40\,\text{mol}
0.40
mol
of
F
e
2
+
\mathrm{Fe^{2+}}
F
e
2
+
is oxidized completely according to this half-reaction? a)
0.80
mol
0.80\,\text{mol}
0.80
mol
b)
1.2
mol
1.2\,\text{mol}
1.2
mol
c)
0.20
mol
0.20\,\text{mol}
0.20
mol
d)
0.40
mol
0.40\,\text{mol}
0.40
mol
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