The effect of temperature on the reaction rate between hydrochloric acid HCl and sodium thiosulphate Na2S2O3 can be explained using the collision theory and the Arrhenius equation. The reaction between HCl and Na2S2O3 is as follows: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 collisions between the reacting particles and the energy with which they collide. As the temperature increases, the kinetic energy of the particles also increases, leading to a higher frequency of collisions and a greater proportion of collisions with sufficient energy to overcome the activation energy barrier.The Arrhenius equation describes 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 e^-Ea/RT becomes larger, leading to an increase in the rate constant k . This means that the reaction rate between hydrochloric acid and sodium thiosulphate will increase with increasing temperature, as more particles have sufficient energy to overcome the activation energy barrier.In summary, the effect of temperature on the reaction rate between hydrochloric acid and sodium thiosulphate is that the rate increases with increasing temperature. This observation is consistent with the Arrhenius equation, which describes the temperature dependence of reaction rates based on the activation energy and the frequency of collisions between reacting particles.