If the concentration of reactants is increased such that one is a limiting agent, wouldn't the concentration of products also increase (because excess of a reactant will get carried to the other(product) side of the equation considering that the limiting agent is in aqueous medium?
e.g.
(Consider 1 mole of each reactant)
HX2O+NHX3−⇀↽−NHX4X++OHX−HX2O+NHX3↽−−⇀NHX4X++OHX−
Now, let us take another scenario in which there are two moles of NH3 and 1 mole of H20. Then concentration of one reactant has increased (from the previous scenario). Wouldn't the concentration of the products also increase because one mole of NH3 does not react and gets carried to the products' side of the equation?
I am confused with how Le Chatelier's principle is applied in the 2nd scenario. Why does the equilibrium shift to the right if the concentration of the reactants and products increase (if my assumption is right)
If my assumption is wrong (concentration of product increases to balance excess reactant), my concern is such an equation is not balanced. I am unable to reconcile how the Le Chatelier's principle is applied in the 2nd scenario.
