The rate of the reaction between hydrochloric acid and sodium thiosulfate typically increases as the temperature increases. This is because an increase in temperature provides the reacting molecules with more kinetic energy, which in turn increases the frequency and energy of collisions between the molecules.The reaction between hydrochloric acid HCl and sodium thiosulfate Na2S2O3 can be represented by the following balanced equation:2HCl aq + Na2S2O3 aq 2NaCl aq + H2O l + SO2 g + S s According to the collision theory, the rate of a chemical reaction depends on the frequency of effective collisions between the reacting molecules. When the temperature increases, the molecules move faster and collide more frequently, leading to a higher probability of effective collisions and thus a faster reaction rate.Additionally, the Arrhenius equation can be used to describe the temperature dependence of reaction rates: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.In summary, the rate of the reaction between hydrochloric acid and sodium thiosulfate generally increases as the temperature increases due to the increased frequency and energy of molecular collisions and the temperature dependence of the rate constant.