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Consider the following generic reaction. A 2 B ( g ) − ⇀ ↽ − 2 A ( g ) + B ( g ) The initial concentration of A 2 B is 0.87 M and the initial concentrations of A and B are assumed to be zero. What is the equilibrium constant expression ( K c ) , if the equilibrium concentration of B is represented by x ?

Respuesta :

Answer : The equilibrium constant expression will be [tex]K_c=\frac{4x^3}{(0.87-x)}[/tex]

Solution :

Equilibrium constant : It is defined as the equilibrium constant. It is defined as the ratio of concentration of products to the concentration of reactants.

The given equilibrium reaction is,

                          [tex]A_2B(g)\rightleftharpoons 2A(g)+B(g)[/tex]

Initially conc.     0.87          0           0

At equilibrium  (0.87-x)      2x          x

The expression of [tex]K_c[/tex] will be,

[tex]K_c=\frac{[A]^2[B]}{[A_2B]}[/tex]

[tex]K_c=\frac{(2x)^2\times (x)}{(0.87-x)}[/tex]

[tex]K_c=\frac{4x^3}{(0.87-x)}[/tex]

Therefore, the equilibrium constant expression will be [tex]K_c=\frac{4x^3}{(0.87-x)}[/tex]

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