A change in temperature can significantly affect the reaction rate of the chemical reaction between potassium permanganate KMnO4 and oxalic acid C2H2O4 in an acidic solution. This reaction is a redox reaction, where potassium permanganate acts as an oxidizing agent and oxalic acid acts as a reducing agent.According to the Collision Theory, an increase in temperature leads to an increase in the kinetic energy of the reacting molecules. As a result, the frequency of collisions between the molecules increases, leading to a higher probability of successful collisions and the formation of products. This, in turn, increases the reaction rate.Furthermore, the Arrhenius equation also describes the relationship between temperature and reaction rate:k = Ae^-Ea/RT where k is the reaction 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.From the Arrhenius equation, it can be seen that an increase in temperature leads to an increase in the reaction rate constant k , which in turn increases the reaction rate.In summary, an increase in temperature will generally lead to an increased reaction rate between potassium permanganate and oxalic acid in an acidic solution, due to the increased frequency of successful molecular collisions and the temperature dependence of the reaction rate constant. Conversely, a decrease in temperature will generally lead to a decreased reaction rate.