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

Answer:

$9.044\times 10^{-3}$ is the value of the equilibrium constant for this reaction at 756 K.

Explanation:

$COCl_2\rightleftharpoons CO+Cl_2$

Equilibrium concentration of $COCl_2$

$[COCl_2]=7.40\times 10^{-4} M$

Equilibrium concentration of $CO$

$[CO]=3.76\times 10^{-2} M$

Equilibrium concentration of $Cl_2$

$[Cl_2]=1.78\times 10^{-4} M$

The expression of an equilibrium constant can be written as;

$K_c=\frac{[CO][Cl_2]}{[COCl_2]}$

$=\frac{3.76\times 10^{-2}\times 1.78\times 10^{-4}}{7.40\times 10^{-4}}$

$K_c=9.044\times 10^{-3}$

$9.044\times 10^{-3}$ is the value of the equilibrium constant for this reaction at 756 K.