The reaction between potassium permanganate KMnO4 and oxalic acid C2H2O4 is a redox reaction in which potassium permanganate acts as an oxidizing agent and oxalic acid acts as a reducing agent. The reaction can be affected by various factors, including temperature, concentration, and light.The effect of different wavelengths of light on the reaction rate between potassium permanganate and oxalic acid can be explained by the concept of photochemistry. Photochemistry is the study of chemical reactions that are influenced by light. When light is absorbed by a molecule, it can cause the molecule to undergo a chemical reaction.In the case of the reaction between potassium permanganate and oxalic acid, different wavelengths of light can have varying effects on the reaction rate. For example, shorter wavelengths of light, such as ultraviolet UV light, have higher energy and can cause the reaction to proceed faster. This is because the higher energy light can excite the molecules, making them more reactive and increasing the rate of the reaction.On the other hand, longer wavelengths of light, such as visible light or infrared IR light, have lower energy and may not have a significant effect on the reaction rate. In some cases, longer wavelengths of light may even slow down the reaction rate, as they can cause the molecules to vibrate or rotate, which can hinder the reaction.In summary, the effect of different wavelengths of light on the reaction rate between potassium permanganate and oxalic acid depends on the energy of the light. Higher energy light, such as UV light, can increase the reaction rate, while lower energy light, such as visible or IR light, may have little to no effect or even slow down the reaction.