To calculate the activation energy Ea of a chemical reaction, we can use the Arrhenius equation:k = A * exp -Ea / R * T 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.Since we have the rate constants at two different temperatures, we can set up two equations:k1 = A * exp -Ea / R * T1 k2 = A * exp -Ea / R * T2 Now, we can divide the first equation by the second equation:k1 / k2 = exp -Ea / R * T1 / exp -Ea / R * T2 Simplify the equation by combining the exponential terms:k1 / k2 = exp Ea / R * 1/T2 - 1/T1 Now, take the natural logarithm of both sides:ln k1 / k2 = Ea / R * 1/T2 - 1/T1 Finally, solve for Ea:Ea = R * ln k1 / k2 / 1/T2 - 1/T1 Plug in the values of k1, k2, T1, and T2 to calculate the activation energy.