The effect of temperature on the rate of the reaction between magnesium and hydrochloric acid can be explained using the Arrhenius equation. The Arrhenius equation is a mathematical formula that describes the temperature dependence of reaction rates. It is given by the following equation:k = Ae^-Ea/RT where:- k is the rate constant of the reaction- A is the pre-exponential factor, which is a constant specific to the reaction- e is the base of the natural logarithm approximately 2.718 - Ea is the activation energy of the reaction in joules per mole - R is the gas constant 8.314 J/molK - T is the temperature in kelvinAs the temperature T increases, the exponential term e^-Ea/RT becomes larger, which in turn increases the rate constant k . This means that the reaction rate between magnesium and hydrochloric acid will increase as the temperature increases.The reason behind this temperature dependence is that, at higher temperatures, the molecules have more kinetic energy, which increases the frequency of collisions between the reactants. Additionally, a greater proportion of these collisions will have enough energy to overcome the activation energy barrier, leading to a higher rate of successful reactions.In summary, the rate of the reaction between magnesium and hydrochloric acid increases with increasing temperature, as described by the Arrhenius equation. This is due to the increased frequency of collisions and the greater proportion of collisions with sufficient energy to overcome the activation energy barrier at higher temperatures.