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Chemistry
Chemistry
Problem
The industrial oxidation of sulfur dioxide is represented by
2
SO
2
(
g
)
+
O
2
(
g
)
→
2
SO
3
(
g
)
Δ
H
rxn
=
−
198
kJ mol
−
1
of SO
3
f
o
r
m
e
d
2\,\text{SO}_2(\text{g}) + \text{O}_2(\text{g}) \rightarrow 2\,\text{SO}_3(\text{g}) \quad \Delta H_{\text{rxn}} = -198\,\text{kJ mol}^{-1}\text{ of SO}_3 formed
2
SO
2
(
g
)
+
O
2
(
g
)
→
2
SO
3
(
g
)
Δ
H
rxn
=
−
198
kJ mol
−
1
of SO
3
f
or
m
e
d
If a plant produces
SO
3
\text{SO}_3
SO
3
at a steady rate of
2.5
mol s
−
1
2.5\,\text{mol s}^{-1}
2.5
mol s
−
1
, determine the rate at which heat is released, in
kJ h
−
1
\text{kJ h}^{-1}
kJ h
−
1
.
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