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Chemistry
Chemistry
Problem
At a certain temperature, the equilibrium constant for the forward reaction below is
K
0
=
2.0
×
10
4
K_0=2.0\times10^{4}
K
0
=
2.0
×
1
0
4
.
2
P
(
g
)
⇌
Q
(
g
)
+
R
(
g
)
2P(g)\rightleftharpoons Q(g)+R(g)
2
P
(
g
)
⇌
Q
(
g
)
+
R
(
g
)
What is the equilibrium constant for the reaction written as
3
Q
(
g
)
+
3
R
(
g
)
⇌
6
P
(
g
)
3Q(g)+3R(g)\rightleftharpoons6P(g)
3
Q
(
g
)
+
3
R
(
g
)
⇌
6
P
(
g
)
a)
K
0
3
K_0^{3}
K
0
3
b)
1
K
0
\dfrac{1}{K_0}
K
0
1
c)
(
1
K
0
)
3
\left(\dfrac{1}{K_0}\right)^{3}
(
K
0
1
)
3
d)
K
0
1
/
3
K_0^{1/3}
K
0
1/3
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