The reaction between potassium permanganate KMnO4 and oxalic acid C2H2O4 in an acidic medium is a redox reaction. In this reaction, potassium permanganate acts as an oxidizing agent, while oxalic acid acts as a reducing agent. The reaction can be represented by the following balanced equation:2 KMnO4 + 5 C2H2O4 + 6 H2SO4 2 MnSO4 + 10 CO2 + 8 H2O + K2SO4Now, let's discuss the effect of light intensity on the rate of this reaction. The reaction between potassium permanganate and oxalic acid in an acidic medium is not a photochemical reaction, meaning it is not directly influenced by light. However, light can have an indirect effect on the reaction rate by affecting the temperature of the reaction mixture.As the intensity of light increases, it can cause an increase in the temperature of the reaction mixture. According to the collision theory, an increase in temperature leads to an increase in the kinetic energy of the reacting particles. This results in more frequent and energetic collisions between the reactant molecules, which in turn increases the rate of the reaction.In summary, while the intensity of light does not directly affect the rate of the reaction between potassium permanganate and oxalic acid in an acidic medium, it can have an indirect effect by influencing the temperature of the reaction mixture. An increase in light intensity can lead to an increase in temperature, which can subsequently increase the rate of the reaction.