Answer: Concentration of
= 0.328 M
Concentration of
= 0.328 M
Concentration of
= 0.532 M
Explanation:
Moles of
and
= 0.430 mole
Volume of solution = 0.500 L
Initial concentration of
and
=![\frac{moles}{volume}=\frac{0.430}{0.500}=0.860M](https://tex.z-dn.net/?f=%5Cfrac%7Bmoles%7D%7Bvolume%7D%3D%5Cfrac%7B0.430%7D%7B0.500%7D%3D0.860M)
The given balanced equilibrium reaction is,
![CO(g)+Cl_2(g)\rightleftharpoons COCl_2(g)](https://tex.z-dn.net/?f=CO%28g%29%2BCl_2%28g%29%5Crightleftharpoons%20COCl_2%28g%29)
Initial conc. 0.860M 0.860M 0
At eqm. conc. (0.860-x) M (0.860-x) M (x) M
The expression for equilibrium constant for this reaction will be,
![K_c=\frac{[COCl_2]}{[CO][Cl_2]}](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7B%5BCOCl_2%5D%7D%7B%5BCO%5D%5BCl_2%5D%7D)
Now put all the given values in this expression, we get :
![4.95=\frac{x}{(0.860-x)^2}](https://tex.z-dn.net/?f=4.95%3D%5Cfrac%7Bx%7D%7B%280.860-x%29%5E2%7D)
By solving the term 'x', we get :
x = 0.532 M
Thus, the concentrations of
at equilibrium are :
Concentration of
= (0.860-x) M =(0.860-0.532) M = 0.328 M
Concentration of
= (0.860-x) M = (0.860-0.532) M = 0.328 M
Concentration of
= x M = 0.532 M