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Chemistry
Chemistry
Problem
The roasting of iron(II) sulfide occurs according to
4
F
e
S
2
+
11
O
2
→
2
F
e
2
O
3
+
8
S
O
2
\mathrm{4\,FeS_2 + 11\,O_2 \rightarrow 2\,Fe_2O_3 + 8\,SO_2}
4
Fe
S
2
+
11
O
2
→
2
F
e
2
O
3
+
8
S
O
2
. A sample containing
25.0
g
\mathrm{25.0\,g}
25.0
g
of
F
e
S
2
\mathrm{FeS_2}
Fe
S
2
is heated in the presence of
20.0
g
\mathrm{20.0\,g}
20.0
g
of
O
2
\mathrm{O_2}
O
2
, and
11.0
g
\mathrm{11.0\,g}
11.0
g
of
S
O
2
\mathrm{SO_2}
S
O
2
is obtained. Calculate the percent yield of
S
O
2
\mathrm{SO_2}
S
O
2
for this reaction.
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