Effect of Increased Reactant on Equilibrium

A chemical equilibrium is reached in a reaction when the rates of the forward and reverse reactions are equal and the concentrations of the reactants and products no longer change. Consider the following equilibrium reaction:

A + B ⇌ C + D

In this reaction, the addition of more reactant A would typically affect the equilibrium position. This change is explained by Le Chatelier's principle, which states that if a system at equilibrium experiences a change in concentration, pressure, or temperature, the equilibrium will shift to counteract that change.

Based on this information, if the concentration of reactant A is increased, what is expected to happen to the concentration of products C and D at equilibrium?