To calculate the activation energy Ea for the oxidation of tin in a solution of hydrochloric acid, we can use the Arrhenius equation:k = A * exp -Ea / R * T where k is the rate constant 5.6 x 10^-3 molL^-1s^-1 , A is the pre-exponential factor, Ea is the activation energy, R is the gas constant 8.314 Jmol^-1K^-1 , and T is the temperature in Kelvin 25C + 273.15 = 298.15 K .However, we don't have enough information to directly calculate the activation energy using the Arrhenius equation, as we don't know the pre-exponential factor A . Alternatively, we can try to use the standard electrode potential E for the Sn2+/Sn couple -0.14 V and the Nernst equation to estimate the activation energy. The Nernst equation is:E = E - RT / nF * ln Q where E is the electrode potential, E is the standard electrode potential, R is the gas constant, T is the temperature in Kelvin, n is the number of electrons transferred in the redox reaction 2 for Sn2+/Sn couple , F is the Faraday constant 96485 Cmol^-1 , and Q is the reaction quotient.However, we still don't have enough information to calculate the activation energy using the Nernst equation, as we don't know the reaction quotient Q and the actual electrode potential E under the given conditions.In summary, we cannot calculate the activation energy for the oxidation of tin in a solution of hydrochloric acid with the given information. We would need additional information, such as the pre-exponential factor A or the reaction quotient Q and the actual electrode potential E under the given conditions.