The effect of temperature on the rate of the photochemical reaction between benzene and chlorine can be explained using the Arrhenius equation and the concept of activation energy.The Arrhenius equation states that the rate constant k of a reaction is related to the temperature T by the following equation:k = Ae^-Ea/RT where A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the temperature in Kelvin.In the photochemical reaction between benzene and chlorine, light usually UV light provides the energy needed to break the Cl-Cl bond in the chlorine molecule, forming two chlorine radicals. These radicals then react with benzene to form chlorobenzene and a hydrogen chloride molecule.The reaction can be represented as:C6H6 + Cl2 + h C6H5Cl + HClAs the temperature increases, the kinetic energy of the molecules also increases, which leads to a higher probability of successful collisions between the reactants. This, in turn, increases the rate of the reaction.However, it is essential to note that the photochemical reaction is primarily driven by the absorption of light energy h rather than thermal energy. Therefore, while an increase in temperature can have some effect on the reaction rate, the primary factor controlling the rate of the photochemical reaction between benzene and chlorine is the intensity and wavelength of the light source.In summary, the effect of temperature on the rate of the photochemical reaction between benzene and chlorine is relatively minor compared to the effect of the light source. However, an increase in temperature can still lead to a higher reaction rate due to increased kinetic energy and a higher probability of successful collisions between the reactant molecules.