To determine the activation energy Ea for the electrochemical reaction between zinc and copper II sulfate solution, we can use the Arrhenius equation:k = A * e^-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.We have two sets of data: k1 = 2.8 x 10^-3 s^-1 at T1 = 298 K, and k2 = 8.7 x 10^-3 s^-1 at T2 = 308 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 Simplifying the equation:k1 / k2 = e^[ Ea / R * 1/T2 - 1/T1 ]Now, we can plug in the given values for k1, k2, T1, and T2: 2.8 x 10^-3 / 8.7 x 10^-3 = e^[ Ea / 8.314 * 1/308 - 1/298 ]0.3218 = e^[ Ea / 8.314 * -0.00322 ]Now, take the natural logarithm of both sides:ln 0.3218 = Ea / 8.314 * -0.00322 -1.134 = Ea / 8.314 * -0.00322 Now, solve for Ea:Ea = -1.134 / -0.00322 * 8.314Ea 2919.6 J/molThe activation energy for the electrochemical reaction between zinc and copper II sulfate solution is approximately 2919.6 J/mol.