The effect of temperature on the reaction rate and sustainability of the reaction between magnesium and hydrochloric acid can be explained using the collision theory and the Arrhenius equation. The reaction between magnesium Mg and hydrochloric acid HCl is an exothermic reaction, which can be represented by the following 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 and energetic collisions between the reacting particles. According to the collision theory, a higher number of effective collisions results in an increased reaction rate.The Arrhenius equation further explains the relationship between temperature and reaction rate: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. As the temperature T increases, the exponential term becomes larger, leading to an increase in the rate constant k and thus a faster reaction rate.However, the sustainability of the reaction depends on the availability of the reactants. In this case, the reaction will continue until either the magnesium or the hydrochloric acid is completely consumed. Increasing the temperature will not affect the sustainability of the reaction in terms of the amount of product formed, but it will cause the reaction to reach completion more quickly.In summary, increasing the temperature will increase the reaction rate between magnesium and hydrochloric acid, but it will not affect the overall sustainability of the reaction in terms of the amount of product formed. The reaction will continue until one of the reactants is completely consumed, and the reaction will reach completion more quickly at higher temperatures.