The reaction between hydrochloric acid HCl and magnesium Mg can be represented by the following balanced chemical equation:Mg s + 2 HCl aq MgCl2 aq + H2 g This reaction is a typical example of an acid-metal reaction, where magnesium displaces hydrogen from hydrochloric acid to form magnesium chloride and hydrogen gas. The rate of this reaction depends on the concentration of hydrochloric acid and the surface area of magnesium.Now, let's consider the effect of increasing the concentration of the product magnesium chloride on the rate of the reaction. According to Le Chatelier's principle, if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust itself to counteract the change and restore a new equilibrium.In this case, if we increase the concentration of magnesium chloride, the system will try to counteract this change by shifting the position of equilibrium to the left, favoring the reverse reaction i.e., the reaction between magnesium chloride and hydrogen gas to form magnesium and hydrochloric acid . However, it is important to note that the reaction between magnesium and hydrochloric acid is essentially a one-way reaction, as the reverse reaction is highly unlikely to occur under normal conditions.Therefore, increasing the concentration of magnesium chloride will have a negligible effect on the rate of the reaction between hydrochloric acid and magnesium. The reaction rate will still primarily depend on the concentration of hydrochloric acid and the surface area of magnesium.