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Chemistry
Chemistry
Problem
At 298 K the following reactions have the indicated standard entropy changes: (1)
2
NO
(
g
)
+
O
2
(
g
)
→
2
NO
2
(
g
)
2\,\text{NO}(g)+\text{O}_{2}(g) \rightarrow 2\,\text{NO}_{2}(g)
2
NO
(
g
)
+
O
2
(
g
)
→
2
NO
2
(
g
)
Δ
S
∘
=
−
146
J mol
−
1
K
−
1
\Delta S^{\circ}= -146\;\text{J mol}^{-1}\text{K}^{-1}
Δ
S
∘
=
−
146
J mol
−
1
K
−
1
(2)
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
S
∘
=
+
24
J mol
−
1
K
−
1
\Delta S^{\circ}= +24\;\text{J mol}^{-1}\text{K}^{-1}
Δ
S
∘
=
+
24
J mol
−
1
K
−
1
Determine
Δ
S
∘
\Delta S^{\circ}
Δ
S
∘
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
)
Give your answer with units.
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