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Chemistry
Chemistry
Problem
Consider the following elementary reactions and their enthalpy changes. 1.
N
2
(
g
)
+
O
2
(
g
)
→
2
NO
(
g
)
\text{N}_2(g) + \text{O}_2(g) \rightarrow 2\,\text{NO}(g)
N
2
(
g
)
+
O
2
(
g
)
→
2
NO
(
g
)
Δ
H
1
=
+
180.5
kJ
\Delta H_1 = +180.5\,\text{kJ}
Δ
H
1
=
+
180.5
kJ
2.
NO
(
g
)
+
1
2
O
2
(
g
)
→
NO
2
(
g
)
\text{NO}(g) + \tfrac{1}{2}\,\text{O}_2(g) \rightarrow \text{NO}_2(g)
NO
(
g
)
+
2
1
O
2
(
g
)
→
NO
2
(
g
)
Δ
H
2
=
−
57.2
kJ
\Delta H_2 = -57.2\,\text{kJ}
Δ
H
2
=
−
57.2
kJ
What is
Δ
H
\Delta H
Δ
H
for the reaction
N
2
(
g
)
+
2
O
2
(
g
)
→
2
NO
2
(
g
)
\text{N}_2(g) + 2\,\text{O}_2(g) \rightarrow 2\,\text{NO}_2(g)
N
2
(
g
)
+
2
O
2
(
g
)
→
2
NO
2
(
g
)
? a)
−
66.1
kJ
-66.1\,\text{kJ}
−
66.1
kJ
b)
+
123.3
kJ
+123.3\,\text{kJ}
+
123.3
kJ
c)
+
66.1
kJ
+66.1\,\text{kJ}
+
66.1
kJ
d)
−
114.4
kJ
-114.4\,\text{kJ}
−
114.4
kJ
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