The rate of reaction between hydrochloric acid and magnesium generally increases with an increase in temperature. This is because, as temperature increases, the kinetic energy of the particles involved in the reaction also increases. This leads to more frequent and energetic collisions between the reactant particles, which in turn increases the probability of successful collisions, resulting in a faster rate of reaction.The reaction between hydrochloric acid HCl and magnesium Mg can be represented by the following balanced chemical equation:Mg s + 2HCl aq MgCl2 aq + H2 g According to the collision theory, the rate of a chemical reaction depends on the frequency and energy of collisions between the reacting particles. When the temperature is increased, the particles move faster and collide more frequently, increasing the likelihood of successful collisions and thus speeding up the reaction rate.It is important to note that the relationship between temperature and reaction rate is not linear. The rate of reaction typically doubles or triples for every 10C increase in temperature, depending on the specific reaction and the activation energy required for the reaction to occur. This relationship can be described by the Arrhenius equation, which relates the rate constant of a reaction to its activation energy and temperature.