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soldi70 [24.7K]
3 years ago
11

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?
Chemistry
1 answer:
o-na [289]3 years ago
5 0

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.

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