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Chemistry
Chemistry
Problem
At 600 K, the equilibrium constant for the reaction
1
2
N
2
(
g
)
+
3
2
H
2
(
g
)
⇌
NH
3
(
g
)
\tfrac12\,\text{N}_2(g)+\tfrac32\,\text{H}_2(g)\rightleftharpoons\text{NH}_3(g)
2
1
N
2
(
g
)
+
2
3
H
2
(
g
)
⇌
NH
3
(
g
)
is
K
1
=
6.0
×
10
2
K_1=6.0\times10^{2}
K
1
=
6.0
×
1
0
2
. What is the value of the equilibrium constant for the reaction written as
N
2
(
g
)
+
3
H
2
(
g
)
⇌
2
NH
3
(
g
)
\text{N}_2(g)+3\,\text{H}_2(g)\rightleftharpoons2\,\text{NH}_3(g)
N
2
(
g
)
+
3
H
2
(
g
)
⇌
2
NH
3
(
g
)
a)
1.2
×
10
3
1.2\times10^{3}
1.2
×
1
0
3
b)
3.6
×
10
4
3.6\times10^{4}
3.6
×
1
0
4
c)
3.6
×
10
5
3.6\times10^{5}
3.6
×
1
0
5
d)
2.5
×
10
1
2.5\times10^{1}
2.5
×
1
0
1
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