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Chemistry
Chemistry
Problem
At 1000 K, the forward reaction has a negative
Δ
G
∘
\Delta G^\circ
Δ
G
∘
value:
2
NO
2
(
g
)
⇌
2
NO
(
g
)
+
O
2
(
g
)
2\text{NO}_2(\text{g}) \rightleftharpoons 2\text{NO}(\text{g}) + \text{O}_2(\text{g})
2
NO
2
(
g
)
⇌
2
NO
(
g
)
+
O
2
(
g
)
Which expression is correct for the equilibrium at this temperature? a.
[
NO
2
]
2
>
[
NO
]
2
[
O
2
]
[\text{NO}_2]^2 > [\text{NO}]^2[\text{O}_2]
[
NO
2
]
2
>
[
NO
]
2
[
O
2
]
b.
[
NO
2
]
<
[
NO
]
[\text{NO}_2] < [\text{NO}]
[
NO
2
]
<
[
NO
]
c.
[
NO
]
=
2
[
O
2
]
[\text{NO}] = 2[\text{O}_2]
[
NO
]
=
2
[
O
2
]
d.
K
>
1
K > 1
K
>
1
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