The temperature has a significant effect on the rate of reaction between sodium thiosulfate Na2S2O3 and hydrochloric acid HCl . As the temperature increases, the rate of reaction also increases. This can be explained by the collision theory and the concept of activation energy.1. Collision theory: According to the collision theory, for a reaction to occur, the reactant particles must collide with each other with sufficient energy and proper orientation. When the temperature increases, the kinetic energy of the particles also increases, causing them to move faster. This results in a higher frequency of collisions between the sodium thiosulfate and hydrochloric acid particles, leading to an increased rate of reaction.2. Activation energy: Activation energy is the minimum amount of energy required for a reaction to occur. When the temperature increases, more particles have enough energy to overcome the activation energy barrier. This results in a higher proportion of successful collisions, which in turn increases the rate of reaction.In summary, an increase in temperature leads to a higher rate of reaction between sodium thiosulfate and hydrochloric acid due to an increased frequency of collisions and a higher proportion of particles with sufficient energy to overcome the activation energy barrier.