To calculate the activation energy Ea of a reaction, we can use the Arrhenius equation:k = A * e^-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/mol*K , and T is the temperature in Kelvin.We have two sets of data: k1 = 8.23 x 10^-4 s^-1 at T1 = 300 K and k2 = 1.56 x 10^-2 s^-1 at T2 = 350 K. We can set up two equations using the Arrhenius equation:k1 = A * e^-Ea / R * T1 k2 = A * e^-Ea / R * T2 Now, we can divide the first equation by the second equation to eliminate the pre-exponential factor A :k1 / k2 = e^-Ea / R * T1 / e^-Ea / R * T2 Simplify the equation: k1 / k2 = e^ -Ea / R * 1/T1 - 1/T2 Take the natural logarithm of both sides:ln k1 / k2 = -Ea / R * 1/T1 - 1/T2 Now, we can solve for Ea:Ea = -R * ln k1 / k2 / 1/T1 - 1/T2 Plug in the given values:Ea = -8.314 J/mol*K * ln 8.23 x 10^-4 s^-1 / 1.56 x 10^-2 s^-1 / 1/300 K - 1/350 K Ea 49050 J/molThe activation energy of the reaction is approximately 49.05 kJ/mol.