Homogeneous Equilibrium: Equilibrium in a system having only one phase is called homogeneous equilibrium.
e. g. N2 (g) + 3H2 (g) ⇌ 2NH3(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 CO2 and H2 at equlibrium.
Hence, equilibrium constant can be written as –
Kc = \(\frac{X^2}{(0.1-X)^2}\) = 4.24
x2 = 4.24(0.01 + x20.2x)
x2 = 0.0424 + 4.25x2 − 0.848x)
3.24x2 − 0848x ± 0.848, c = 0.0424
For quadratic equation ax2 + bx + c = 0
x = \( {(-b \pm \sqrt{b^2-4ac}) \over 2a}\)
x = \( {(0.848 \pm \sqrt{(0.848)^2-4\times3.24\times0.0424}) \over 2\times3.24}\)
= \(\frac{0.848 \pm 0.4118}{6.48}\)
x1 = \(\frac{0.848 \pm 0.4118}{6.48}\) = 0.067
x2 = \(\frac{0.848 \pm 0.4118}{6.48}\) = 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 –
[CO2] = [H2] = x = 0.067 M
= [CO] = [H2O] = 0.1 - x
= 0.1 - 0.067
= 0.033 M
(c) For liquid ⇌ vapour equilibrium, the vapour pressure is constant at a given temperature.