The reaction between magnesium and hydrochloric acid is an exothermic reaction, which produces hydrogen gas. The reaction can be represented by the following equation:Mg s + 2HCl aq MgCl2 aq + H2 g The effect of a 10C increase in temperature on the reaction rate can be estimated using the Arrhenius equation, which relates the rate constant k of a reaction to its activation energy Ea and temperature T :k = Ae^-Ea/RT where A is the pre-exponential factor, R is the gas constant 8.314 J/molK , and T is the temperature in Kelvin.According to the Arrhenius equation, increasing the temperature will increase the reaction rate. This is because higher temperatures provide more energy to the reacting molecules, allowing them to overcome the activation energy barrier more easily.To estimate the effect of a 10C increase in temperature on the reaction rate, we can use the rule of thumb that the reaction rate approximately doubles for every 10C increase in temperature. This is a rough estimate and may not be accurate for all reactions, but it can give us an idea of the effect of temperature on the reaction rate.So, for the reaction between magnesium and hydrochloric acid, a 10C increase in temperature would roughly double the reaction rate. This means that the volume of hydrogen gas produced in 5 minutes would also approximately double, assuming that the reaction is limited by the reaction rate and not by the availability of reactants.