To calculate the activation energy Ea of a reaction, 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.However, we don't have enough information to directly use the Arrhenius equation. Instead, we can use the temperature coefficient Q10 to find the activation energy. The Q10 is the factor by which the reaction rate increases for every 10C increase in temperature:Q10 = k2 / k1 ^10 / T2 - T1 where k1 and k2 are the rate constants at temperatures T1 and T2, respectively. In this case, we have the rate constant at 25C k1 = 3.42 x 10^-3 s^-1 and the temperature coefficient Q10 = 1.99 . We can assume that k2 is the rate constant at 35C T2 = 308.15 K , and T1 is 25C 298.15 K .1.99 = k2 / 3.42 x 10^-3 s^-1 ^10 / 308.15 K - 298.15 K Solving for k2:k2 = 1.99^1 * 3.42 x 10^-3 s^-1 = 6.81 x 10^-3 s^-1Now we have the rate constants at two different temperatures. We can use the Arrhenius equation to find the activation energy:k1 = A * e^-Ea / R * T1 k2 = A * e^-Ea / R * T2 Divide the first equation by the second equation: k1 / k2 = e^ Ea / R * T2 - Ea / R * T1 Take the natural logarithm of both sides:ln k1 / k2 = Ea / R * T2 - Ea / R * T1 Rearrange the equation to solve for Ea:Ea = R * ln k1 / k2 / 1/T1 - 1/T2 Plug in the values:Ea = 8.314 J/molK * ln 3.42 x 10^-3 s^-1 / 6.81 x 10^-3 s^-1 / 1/298.15 K - 1/308.15 K Ea 48,200 J/molThe activation energy of the reaction between hydrochloric acid and zinc is approximately 48,200 J/mol.