The activation energy Ea for the electrochemical reaction between zinc and hydrochloric acid can be determined using 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.The reaction between zinc and hydrochloric acid is as follows:Zn s + 2HCl aq ZnCl2 aq + H2 g To determine the activation energy, we need experimental data on the rate constant k at different temperatures. Unfortunately, without this data, we cannot calculate the activation energy directly. However, we can provide some general information about the reaction.The reaction between zinc and hydrochloric acid is a redox reaction, where zinc is oxidized and hydrogen ions are reduced. The standard reduction potentials for the half-reactions are:Zn2+ + 2e- Zn s E = -0.76 V2H+ + 2e- H2 g E = 0.00 VThe overall cell potential Ecell can be calculated using the Nernst equation:Ecell = Ecathode - EanodeFor this reaction:Ecell = 0.00 V - -0.76 V = 0.76 VThe cell potential is positive, indicating that the reaction is spontaneous at standard conditions. However, this does not provide the activation energy directly.In summary, without experimental data on the rate constant at different temperatures, we cannot calculate the activation energy for the electrochemical reaction between zinc and hydrochloric acid. However, we can determine that the reaction is spontaneous at standard conditions based on the standard reduction potentials.