Question

The molar concentrations for the reactants and products at equilibrium are found to be [CCl4]=1.0 M, [O2]=0.3 M, [COCl2]=4.0 M, and [Cl2]=2.0 M. What is the value of the equilibrium constant for this reaction? 2CCl4(g)+O2(g)⇌2COCl2(g)+2Cl2(g) Express your answer numerically using two significant figures.

Answer 1

`2.1* 10^2` is the value of the equilibrium constant for this reaction.

Step-by-step explanation:

`2CCl_4(g)+O_2(g)\rightleftharpoons 2COCl_2(g)+2Cl_2(g)`

Molar concentrations of
`CCl_4` at equilibrium =
`[CCl_4]=1.0M`

Molar concentrations of
`O_2` at equilibrium =
`[O_2]=0.3M`

Molar concentrations of
`COCl_2` at equilibrium =
`[COCl_2]=4.0M`

Molar concentrations of
`Cl_2` at equilibrium =
`[Cl_2]=2.0M`

The equilibrium constant is given as:

`K_c=([COCl_2]^2[Cl_2]^2)/([CCl_4]^2[O_2])=((4.0 M)^2* (2.0M)^2)/((1.0M)^2* (0.3 M))`

`K_c=213.33\approx 2.1* 10^2`

`2.1* 10^2` is the value of the equilibrium constant for this reaction.