Question

What concentration of Cl2O remains after a mixture that initially contains [H2O] = 1.00 M and [Cl2O] = 1.00 M comes to equilibrium at 25 °C ? Kc for the reaction is 0.0900.

Answer 1

Equilibrium concentration of
`Cl_2O` is 0.870 M.

Step-by-step explanation:

Initial concentration of water =
`[H_2O]=1.00 M`

Initial concentration of
`Cl_2O=[Cl_2O]=1.00 M`

`H_2O(g) + Cl_2O(g)\rightarrow 2HOCl(g), Kc = 0.0900`

initially

1.00 M 1.00 M 0

At equilibrium

(1.00m-x) M (1.00-x)M 2x

The expression of equilibrium constant is given by :

`K_c=([HOCl]^2)/([H_2O][Cl_2O])`

`0.0900=((2x)^2)/((1.00-x)(1.00-x))`

Solving for x :

x = 0.130

Equilibrium concentration of
`Cl_2O`:

`[Cl_2O]=(1,00-x) M=1.00 M-0.130 M=0.870 M`