Temperature plays a significant role in the reaction rate and overall efficiency of the reaction between hydrochloric acid HCl and magnesium ribbon Mg . This reaction can be represented by the following balanced chemical equation:Mg s + 2HCl aq MgCl2 aq + H2 g The reaction rate is influenced by temperature due to the collision theory, which states that for a reaction to occur, particles must collide with the correct orientation and with sufficient energy activation energy . As temperature increases, the kinetic energy of the particles also increases, leading to more frequent and energetic collisions between the reactants.According to the Arrhenius equation, the reaction rate increases exponentially with temperature:k = Ae^-Ea/RT where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the temperature in Kelvin.In the case of the reaction between HCl and Mg, increasing the temperature will lead to a faster reaction rate, as the HCl and Mg particles will collide more frequently and with greater energy. This will result in a more rapid production of magnesium chloride MgCl2 and hydrogen gas H2 .However, it is important to note that increasing the temperature can also affect the overall efficiency of the reaction. Higher temperatures can cause the reactants and products to become more unstable, potentially leading to side reactions or decomposition. In the case of the HCl and Mg reaction, the reactants are relatively stable, and the reaction is relatively simple, so the overall efficiency is not likely to be significantly impacted by temperature changes within a reasonable range.In summary, increasing the temperature will generally lead to a faster reaction rate between hydrochloric acid and magnesium ribbon, while the overall efficiency of the reaction may not be significantly affected within a reasonable temperature range. However, extreme temperatures could potentially impact the stability of the reactants and products, leading to side reactions or decomposition.