The effect of temperature on the rate of reaction between sodium thiosulphate Na2S2O3 and hydrochloric acid HCl can be explained by the collision theory. As the temperature increases, the kinetic energy of the particles also increases, leading to more frequent and energetic collisions between the reactant molecules. This results in an increased rate of reaction.The relationship between the rate of reaction and temperature can be quantified using the Arrhenius equation, which is given by:k = Ae^-Ea/RT where:- k is the rate constant of the reaction- A is the pre-exponential factor or the frequency factor, which represents the rate constant at an infinite temperature- Ea is the activation energy of the reaction, which is the minimum energy required for the reaction to occur- R is the gas constant 8.314 J/mol K - T is the temperature in KelvinTo determine the effect of temperature on the rate of reaction between sodium thiosulphate and hydrochloric acid using the Arrhenius equation, you would need to perform a series of experiments at different temperatures and measure the corresponding rate constants k . By plotting the natural logarithm of the rate constant ln k against the inverse of the temperature 1/T , you can obtain a straight line with a slope equal to -Ea/R. From this, you can calculate the activation energy Ea and the pre-exponential factor A .In summary, the rate of reaction between sodium thiosulphate and hydrochloric acid increases with temperature, and this relationship can be quantified using the Arrhenius equation. By performing experiments at different temperatures and analyzing the data, you can determine the activation energy and the pre-exponential factor for the reaction.