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 The rate of this reaction depends on several factors, including the concentration of the reactants. According to the collision theory, an increase in the concentration of the reactants leads to an increase in the frequency of collisions between the reacting particles, which in turn increases the rate of the reaction.In the case of the reaction between hydrochloric acid and magnesium, increasing the concentration of HCl will increase the rate of the reaction. This is because there will be more HCl molecules available to collide with the magnesium atoms, leading to a faster production of magnesium chloride MgCl2 and hydrogen gas H2 .However, it is important to consider the effect of these changes on the resulting profitability. Increasing the concentration of HCl may lead to higher costs due to the increased amount of raw materials needed. Additionally, a faster reaction rate may require more advanced or expensive equipment to handle the increased production rate and to safely manage the release of hydrogen gas.To maximize profitability, it is crucial to find the optimal balance between the concentration of reactants, the rate of the reaction, and the associated costs. This can be achieved through experimentation and cost analysis, taking into account factors such as raw material costs, equipment costs, labor costs, and the market value of the products MgCl2 and H2 .In summary, increasing the concentration of reactants, such as HCl in the reaction with magnesium, will increase the rate of the reaction. However, the resulting profitability depends on finding the optimal balance between reactant concentrations, reaction rate, and associated costs.