The reaction between hydrogen peroxide H2O2 and potassium iodide KI is a well-known example of a redox reaction, where hydrogen peroxide is reduced to water and iodide ions are oxidized to iodine. This reaction can be affected by various factors, including temperature, concentration, and the presence of catalysts. In this case, we will discuss the effect of different wavelengths of light on the reaction rate and its relation to the activation energy.Different wavelengths of light carry different amounts of energy. In general, shorter wavelengths such as ultraviolet light carry more energy, while longer wavelengths such as infrared light carry less energy. When light interacts with a chemical reaction, it can provide energy to the reactants, potentially increasing the reaction rate.In the case of the H2O2-KI reaction, the activation energy is the minimum amount of energy required for the reaction to proceed. If the energy provided by the light is sufficient to overcome the activation energy barrier, the reaction rate will increase. Conversely, if the energy provided by the light is not enough to overcome the activation energy, the reaction rate will not be significantly affected.The effect of different wavelengths of light on the H2O2-KI reaction can be studied experimentally by exposing the reaction mixture to light sources with varying wavelengths and measuring the reaction rate. It is expected that shorter wavelengths, which carry more energy, will have a greater impact on the reaction rate compared to longer wavelengths.In summary, the effect of different wavelengths of light on the rate of the reaction between hydrogen peroxide and potassium iodide solution is related to the energy carried by the light and the activation energy of the reaction. Shorter wavelengths, which carry more energy, are more likely to increase the reaction rate by providing enough energy to overcome the activation energy barrier.