For any reversible reaction, if concentration of reactants increases, then effect on equilibrium constant :

Increasing the concentration of reactants shifts the equilibrium position forward (more products form), as predicted by Le Chatelier's principle.
However, the concentrations readjust so that the ratio $\dfrac{[\text{products}]}{[\text{reactants}]}$ returns to the same value. The equilibrium constant itself does not change.
The equilibrium constant changes only with temperature.
So the equilibrium constant remains unchanged.