The effect of temperature on the rate and efficiency of the reaction between magnesium and hydrochloric acid can be explained using the collision theory and the concept of activation energy. The reaction between magnesium and hydrochloric acid is an exothermic reaction that produces hydrogen gas, as shown in the balanced chemical equation:Mg s + 2HCl aq MgCl2 aq + H2 g As the temperature increases, the kinetic energy of the particles molecules and ions involved in the reaction also increases. This leads to more frequent collisions between the reacting particles, as well as a higher proportion of these collisions having enough energy to overcome the activation energy barrier for the reaction to occur.As a result, the rate of the reaction between magnesium and hydrochloric acid increases with increasing temperature. This means that the production of hydrogen gas will be faster at higher temperatures compared to lower temperatures.However, it is important to note that the efficiency of the reaction, in terms of the yield of hydrogen gas, is not significantly affected by temperature. This is because the reaction between magnesium and hydrochloric acid is a stoichiometric reaction, meaning that the amount of hydrogen gas produced is directly proportional to the amount of magnesium and hydrochloric acid used. Therefore, as long as the reaction goes to completion, the efficiency of hydrogen gas production remains constant regardless of the temperature.In summary, increasing the temperature of the reaction between magnesium and hydrochloric acid will result in a faster rate of hydrogen gas production, but the overall efficiency of the reaction in terms of hydrogen gas yield remains constant.