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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?

Respuesta :

Answer:

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

Explanation:

[tex]COCl_2\rightleftharpoons CO+Cl_2[/tex]

Equilibrium concentration of [tex]COCl_2[/tex]

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

Equilibrium concentration of [tex]CO[/tex]

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

Equilibrium concentration of [tex]Cl_2[/tex]

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

The expression of an equilibrium constant can be written as;

[tex]K_c=\frac{[CO][Cl_2]}{[COCl_2]}[/tex]

[tex]=\frac{3.76\times 10^{-2}\times 1.78\times 10^{-4}}{7.40\times 10^{-4}}[/tex]

[tex]K_c=9.044\times 10^{-3}[/tex]

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

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