The effect of light intensity on the rate of reaction between potassium permanganate KMnO4 and oxalic acid C2H2O4 is not significant. This reaction is primarily driven by the concentration of the reactants, temperature, and presence of a catalyst, rather than light intensity.The reaction between potassium permanganate and oxalic acid is a redox reaction, where potassium permanganate acts as an oxidizing agent and oxalic acid acts as a reducing agent. The reaction can be represented by the following balanced equation:2 KMnO4 aq + 5 C2H2O4 aq + 3 H2SO4 aq K2SO4 aq + 2 MnSO4 aq + 10 CO2 g + 8 H2O l In this reaction, the potassium permanganate is reduced to manganese sulfate MnSO4 , while the oxalic acid is oxidized to carbon dioxide CO2 and water H2O . The reaction rate is mainly influenced by the concentration of the reactants, temperature, and the presence of a catalyst such as sulfuric acid, H2SO4 .However, light intensity does not play a significant role in this reaction. In some photochemical reactions, light can provide the energy needed to break chemical bonds and initiate the reaction, but this is not the case for the reaction between potassium permanganate and oxalic acid. The reaction proceeds spontaneously in the presence of a catalyst and does not require light energy to proceed.