**Homogeneous Equilibrium:** Equilibrium in a system having only one phase is called homogeneous equilibrium.

**e. g.** N_{2} (g) + 3H_{2} (g) ⇌ 2NH_{3}(g)

**(b) For the reaction,**

Let x mole L^{−1} of each the product be formed

At equilibrium (0.1- x) M (0.1 - x) M xM xM where x = amount of CO_{2} and H_{2} at equlibrium.

**Hence, equilibrium constant can be written as –**

K_{c} = \(\frac{X^2}{(0.1-X)^2}\) = 4.24

x^{2} = 4.24(0.01 + x^{2}0.2x)

x^{2 }=^{ }0.0424 + 4.25x^{2} − 0.848x)

3.24x^{2} − 0848x ± 0.848, c = 0.0424

For quadratic equation ax^{2} + bx + c = 0

x = \( {(-b \pm \sqrt{b^2-4ac}) \over 2a}\)

x = \( {(0.848 \pm \sqrt{(0.848)^2-4\times3.24\times0.0424}) \over 2\times3.24}\)

= \(\frac{0.848 \pm 0.4118}{6.48}\)

x_{1} = \(\frac{0.848 \pm 0.4118}{6.48}\) = 0.067

x_{2} = \(\frac{0.848 \pm 0.4118}{6.48}\) = 0.194

The value 0.194 should be neglected because it will give concentration of the reactant which is more than initial concentration. There, the equilibrium concentrations ate –

[CO_{2}] = [H_{2}] = x = 0.067 M

= [CO] = [H_{2}O] = 0.1 - x

= 0.1 - 0.067

= 0.033 M

**(c)** **For liquid** ⇌ vapour equilibrium, the vapour pressure is constant at a given temperature.