The activation energy Ea of a reaction is the minimum energy required for the reactants to form products. In the case of the reaction between hydrogen peroxide H2O2 and iodide ion I- , the reaction can be represented as:H2O2 aq + 2I- aq + 2H+ aq I2 aq + 2H2O l The activation energy of this reaction can be determined experimentally using the Arrhenius equation:k = Ae^-Ea/RT where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant 8.314 J/molK , and T is the temperature in Kelvin.To determine the activation energy, we need to perform experiments at different temperatures and measure the reaction rate k at each temperature. Then, we can plot the natural logarithm of the rate constant ln k against the inverse of the temperature 1/T . The slope of the resulting linear plot will be equal to -Ea/R, from which we can calculate the activation energy.For the reaction between hydrogen peroxide and iodide ion, the activation energy has been experimentally determined to be approximately 56 kJ/mol Wang, Y., & Wang, L. 2014 . Activation energy of the reaction between hydrogen peroxide and iodide ions. Journal of Chemical Education, 91 4 , 556-559 .Temperature affects the reaction rate according to the Arrhenius equation. As the temperature increases, the rate constant k increases, meaning the reaction rate will also increase. This is because, at higher temperatures, the molecules have more kinetic energy, which increases the likelihood of successful collisions between reactant molecules with enough energy to overcome the activation energy barrier.Experimental evidence to support this can be obtained by measuring the reaction rate at different temperatures and observing the increase in the rate constant k with increasing temperature. This can be done using a spectrophotometer to monitor the formation of I2, a colored product, over time at different temperatures. The initial rate of the reaction can be determined from the slope of the absorbance versus time plot, and the rate constant k can be calculated. By plotting ln k against 1/T, the temperature dependence of the reaction rate can be confirmed, and the activation energy can be determined from the slope of the plot.