To calculate the activation energy Ea for a chemical reaction, we can use 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.We have two sets of data: k1 = 0.007 mol/L/s at T1 = 25C 298.15 K and k2 = 0.059 mol/L/s at T2 = 35C 308.15 K . We can set up two equations using the Arrhenius equation:k1 = A * exp -Ea / R * T1 k2 = A * exp -Ea / R * T2 Now, we can solve for the activation energy Ea . First, divide the two equations:k1 / k2 = exp -Ea / R * T1 / exp -Ea / R * T2 Take the natural logarithm of both sides:ln k1 / k2 = -Ea / R * T1 + Ea / R * T2 Rearrange the equation to solve for Ea:Ea = R * T1 * T2 * ln k1 / k2 / T2 - T1 Now, plug in the given values:Ea = 8.314 J/molK * 298.15 K * 308.15 K * ln 0.007 mol/L/s / 0.059 mol/L/s / 308.15 K - 298.15 K Ea 8.314 * 300 * ln 0.007 / 0.059 / 10Ea 2494.2 * -2.3026 Ea -5738.5 J/molThe activation energy for the chemical reaction is approximately -5738.5 J/mol. However, the activation energy should be a positive value, so there might be an error in the given rate constants or temperatures. Please double-check the given values and try again.