$2\mathrm{HI}\left(g\right)\rightleftharpoons {\mathrm{H}}_2\left(g\right)+{\mathrm{I}}_2\left(g\right)$ The equilibrium constant for the above reaction is 6.4 at 300 K. If 0.25 mole each of H₂ and I₂ are added to the system, the equilibrium constant will be:

The equilibrium constant of the above reaction is 6.4 at 300K. If 0.25mole each of H_2​ and I₂​ are added to the system, the equilibrium constant will be 6.4.
 Equilibrium constant depends on temperature and is independent of the actual quantities of reactants and products, the presence of a catalyst and the presence of inert material. It is also independent of concentrations, pressures and volumes of reactants and products.