The formation of reaction products can affect the rate of the chemical reaction between hydrochloric acid HCl and magnesium ribbon Mg in several ways. The reaction between HCl and Mg can be represented by the following balanced equation:Mg s + 2HCl aq MgCl2 aq + H2 g As the reaction proceeds, magnesium reacts with hydrochloric acid to form magnesium chloride MgCl2 and hydrogen gas H2 . The rate of this reaction can be influenced by factors such as concentration, temperature, surface area, and the presence of catalysts. Here, we will focus on the formation of reaction products and its effect on the reaction rate.1. Decrease in reactant concentration: As the reaction proceeds and more products are formed, the concentration of the reactants Mg and HCl decreases. According to the collision theory, the rate of a reaction is directly proportional to the concentration of the reactants. As the concentration of reactants decreases, the frequency of effective collisions between the reactant particles also decreases, leading to a slower reaction rate.2. Formation of a protective layer: In some cases, the formation of a reaction product can create a protective layer on the surface of the reactant, which can hinder the reaction. However, in the case of the reaction between HCl and Mg, the product MgCl2 is soluble in water and does not form a protective layer on the magnesium ribbon. Therefore, this factor does not play a significant role in this specific reaction.3. Gas formation: The formation of hydrogen gas H2 can affect the reaction rate by creating bubbles on the surface of the magnesium ribbon. These bubbles can temporarily reduce the surface area of the magnesium ribbon that is in contact with the hydrochloric acid, which may slow down the reaction rate. However, as the bubbles rise and escape from the solution, the surface area is restored, and the reaction rate can increase again.In summary, the formation of reaction products in the reaction between hydrochloric acid and magnesium ribbon mainly affects the reaction rate by decreasing the concentration of the reactants. As the reaction progresses and more products are formed, the reaction rate will gradually decrease due to the reduced concentration of reactants.