Group 2 The equilibrium constant, K, for the following reaction is 1.34E-2 at 60
ID: 880694 • Letter: G
Question
Group 2
The equilibrium constant, K, for the following reaction is 1.34E-2 at 601 K.
COCl2(g) CO(g) + Cl2(g)
An equilibrium mixture of the three gases in a 10.9 L container at 601 K contains 0.265 M COCl2, 5.96E-2 M CO and 5.96E-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the equilibrium mixture is compressed at constant temperature to a volume of 6.29 L?
[COCl2]
=
M
[CO]
=
M
[Cl2]
=
M
The equilibrium constant, K, for the following reaction is 1.88E-2 at 611 K.
COCl2(g) CO(g) + Cl2(g)
An equilibrium mixture of the three gases in a 8.59 L container at 611 K contains 0.273 M COCl2, 7.17E-2 M CO and 7.17E-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if the volume of the container is increased to 19.0 L?
[COCl2]
=
M
[CO]
=
M
[Cl2]
=
M
Explanation / Answer
after decreasing volume to 6.29 L concentration will increase
M1V1=M2V2 relation we can use
[COCl2]=0.45M
[CO]=0.1032M
[Cl2]=0.1032M
after increasing volume to 19.0L the concentration will decrease
M1V1=M2V2 relation we can use
[COCl2]=0.120M
[CO]=0.0324M
[Cl2]=0.0324M
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