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g Potassium chlorate decomposes to product potassium chloride and oxygen gas. 2KClO3(s) ⇔ 2KCl(s) + 3O2(g) When this reaction was run at room temperature, the following equilbrium concentrations were measured: [O2] = 0.0500 M; [KCl] = 0.00250 M; [KClO3] = 2.00 M What is the equilibrium constant for this reaction?

Respuesta :

Answer:

[tex]1.95\times 10^{-10}[/tex] is the equilibrium constant for this reaction.

Explanation:

Equilibrium concentrations were measured:

[tex][O_2] = 0.0500 M[/tex]

[tex] [KCl] = 0.00250 M[/tex]

[tex] [KClO_3] = 2.00 M [/tex]

[tex]2KClO_3(s)\rightleftharpoons 2KCl(s) + 3O_2(g)[/tex]

The expression of an equilibrium constant is given by :

[tex]K_c=\frac{[KCl]^2[O_2]^3}{[KClO_3]^2}[/tex]

[tex]=\frac{[0.00250 M]^2[0.0500 M]^3}{[2.00 M]^2}[/tex]

[tex]K_c=1.95\times 10^{-10}[/tex]

[tex]1.95\times 10^{-10}[/tex] is the equilibrium constant for this reaction.

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