The rate of the reaction between hydrochloric acid HCl and magnesium metal Mg generally increases with increasing temperature. This is because, according to the Collision Theory, an increase in temperature leads to an increase in the kinetic energy of the reacting particles HCl and Mg . As a result, the particles move faster and collide more frequently with greater energy.When the temperature increases, more of these collisions have enough energy to overcome the activation energy barrier, which is the minimum energy required for a successful reaction to occur. Consequently, the number of successful collisions per unit time increases, leading to a faster reaction rate.In summary, the rate of the reaction between hydrochloric acid and magnesium metal increases with increasing temperature due to the increased frequency and energy of collisions between the reacting particles.