Answer: The value of equilibrium constant for the given reaction at 517 K is 1.30
Explanation:
The chemical equation for the dissociation of [tex]CH_2Cl_2[/tex] follows:
[tex]2CH_2Cl_2(g)\rightleftharpoons CH_4(g)+CCl_4(g)[/tex]
The expression of [tex]K_{eq}[/tex] for above equation follows:
[tex]K_{eq}=\frac{[CH_4][CCl_4]}{[CH_2Cl_2]^2}[/tex]
We are given:
[tex][CH_4]_{eq}=3.69\times 10^{-2}M[/tex]
[tex][CCl_4]_{eq}=4.12\times 10^{-2}M[/tex]
[tex][CH_2Cl_2]_{eq}=3.42\times 10^{-2}M[/tex]
Putting values in above expression, we get:
[tex]K_{eq}=\frac{(3.69\times 10^{-2})\times (4.12\times 10^{-2})}{(3.42\times 10^{-2})^2}\\\\K_{eq}=1.30[/tex]
Hence, the value of equilibrium constant for the given reaction at 517 K is 1.30
