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Chemistry
Chemistry
Problem
Hydrazine,
N
2
H
4
\text{N}_2\text{H}_4
N
2
H
4
, is used as a rocket fuel. It reacts according to the thermochemical equation:
N
2
H
4
(
l
)
+
O
2
(
g
)
→
N
2
(
g
)
+
2
H
2
O
(
l
)
Δ
H
⊖
=
−
623
kJ mol
−
1
\text{N}_2\text{H}_4(\text{l}) + \text{O}_2(\text{g}) \rightarrow \text{N}_2(\text{g}) + 2\text{H}_2\text{O}(\text{l}) \quad \Delta H^\ominus = -623 \text{ kJ mol}^{-1}
N
2
H
4
(
l
)
+
O
2
(
g
)
→
N
2
(
g
)
+
2
H
2
O
(
l
)
Δ
H
⊖
=
−
623
kJ mol
−
1
Hydrazine does not, however, burn spontaneously in oxygen. What is the best explanation for this?
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