The rate of the chemical reaction between hydrochloric acid HCl and sodium thiosulphate Na2S2O3 is affected by temperature, as is the case with most chemical reactions. The reaction between HCl and Na2S2O3 produces sodium chloride NaCl , sulfur dioxide SO2 , water H2O , and sulfur S .The reaction rate generally increases with temperature due to the increased kinetic energy of the reacting molecules. As the temperature rises, the molecules move faster, collide more frequently, and with greater energy, which increases the likelihood of successful collisions and the formation of product molecules.According to the Arrhenius equation, the rate constant k of a reaction is related to temperature T by the following equation:k = Ae^-Ea/RT where 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 increases, the exponential term becomes larger, leading to an increase in the rate constant and, consequently, the reaction rate.The specific temperature range that yields the fastest reaction rate depends on the activation energy and other factors specific to the reaction. However, in general, the reaction rate will continue to increase with temperature until it reaches a point where the reactants or the reaction system becomes unstable or the reaction rate is limited by other factors, such as diffusion or the availability of reactants.For the reaction between hydrochloric acid and sodium thiosulphate, the fastest reaction rate is typically observed at temperatures between 40C and 60C. Beyond this range, the reaction rate may continue to increase, but the risk of side reactions, reactant degradation, or other limiting factors may become more significant.