Question

Some COCl2 is placed in a sealed flask and heated to 756 K. When equilibrium is reached, the flask is found to contain COCl2 (7.40×10-4 M), CO (3.76×10-2 M), and Cl2 (1.78×10-2 M). What is the value of the equilibrium constant for this reaction at 756 K?

Answer 1

`9.044* 10^(-3)` is the value of the equilibrium constant for this reaction at 756 K.

Step-by-step explanation:

`COCl_2\rightleftharpoons CO+Cl_2`

Equilibrium concentration of
`COCl_2`

`[COCl_2]=7.40* 10^(-4) M`

Equilibrium concentration of
`CO`

`[CO]=3.76* 10^(-2) M`

Equilibrium concentration of
`Cl_2`

`[Cl_2]=1.78* 10^(-4) M`

The expression of an equilibrium constant can be written as;

`K_c=([CO][Cl_2])/([COCl_2])`

`=(3.76* 10^(-2)* 1.78* 10^(-4))/(7.40* 10^(-4))`

`K_c=9.044* 10^(-3)`

`9.044* 10^(-3)` is the value of the equilibrium constant for this reaction at 756 K.