For the reaction,

Initial concentration:
<u>0.1M</u> , <u>0.1M</u> , <u>0</u> , <u>0</u>
Let 'x' mole per litre of each of theproduct be formed.
At equilibrium:
<u>(0.1 – x)M</u> , <u>(0.1 – x)M</u> , <u>xM</u> , <u>xM</u>
where x is the amount of Carbon dioxide and Hydrogen, at equilibrium.
Hence, equilibrium constant can be written as,

→ x² = 4.24 (0.01 + x² – 0.2x)
→ x² = 0.0424 + 4.24 x² - 0.848x
→ 3.24x² - 0.848x + 0.0424 = 0
<em>a = 3.24, b = -0.848, c = 0.0424</em>
(for quadratic equation ax² + bx+c=0)





Here, the value 0.194 should be neglected because it will give concentration of the reactant which is more than initial concentration.
∴ The equilibrium concentrations are :-
![[CO_2] [H_2] = x = 0.067M](https://tex.z-dn.net/?f=%5BCO_2%5D%20%5BH_2%5D%20%3D%20x%20%3D%200.067M)
![[CO] [H_2 O] = 0.1 - 0.067 = 0.033M](https://tex.z-dn.net/?f=%5BCO%5D%20%5BH_2%20O%5D%20%3D%200.1%20-%200.067%20%3D%200.033M)