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Consider the reaction below. At 500 K, the reaction is at equilibrium with the following concentrations. [PCI5]= 0.0095 M [PCI3] = 0.020 [CI2] = 0.020 M What is the equilibrium constant for the given reaction?

Respuesta :

Answer: The equilibrium constant for the given reaction is 0.0421.

Explanation:

[tex]PCl_5\rightleftharpoons PCl_3+Cl_2[/tex]

Concentration of [tex][PCl_5][/tex] =  0.0095 M

Concentration of [tex][PCl_3][/tex] =  0.020 M

Concentration of [tex][Cl_2][/tex] =  0.020 M

The expression of the equilibrium constant is given as:

[tex]K_c=\frac{[PCl_3][Cl_2]}{[PCl_5]}=\frac{0.020 M\times 0.020 M}{0.0095 M}[/tex]

[tex]K_c=0.0421[/tex] (An equilibrium constant is an unit less constant)

The equilibrium constant for the given reaction is 0.0421.

Answer: 0.042

Explanation:- Equilibrium constant is the ratio of concentration of products to the concentration of reactants each term raised to their stochiometric coefficients.

[tex]PCl_5(g)\rightarrow PCl_3(g)+Cl_2(g)[/tex]

[tex]K_c=\frac{[PCl_3][Cl_2]}{[PCl_5]}[/tex]

Given :[tex][PCl_5][/tex]= 0.0095 M

[tex][PCl_3][/tex] = 0.020 M

[tex][Cl_2][/tex] = 0.020 M

Putting the given values n the equation:

[tex]K_c=\frac{[0.020][0.020]}{[0.0095]}=0.042[/tex]