The alkaline hydrolysis of ethyl ethanoate is a second-order reaction. The rate constant, kkk, for this reaction varies with temperature according to the Arrhenius equation:
k=Ae−EaRTk = A \mathrm{e}^{-\frac{E_{\mathrm{a}}}{RT}}k=Ae−RTEa
At 40 ∘C40\text{ }^\circ\text{C}40 ∘C, the rate constant for this hydrolysis is 5.28×10−3 dm3 mol−1 s−15.28 \times 10^{-3}\text{ dm}^3\text{ mol}^{-1}\text{ s}^{-1}5.28×10−3 dm3 mol−1 s−1. The activation energy for the reaction is 82.4 kJ mol−182.4\text{ kJ mol}^{-1}82.4 kJ mol−1. The gas constant R=8.31 J K−1 mol−1R = 8.31\text{ J K}^{-1}\text{ mol}^{-1}R=8.31 J K−1 mol−1.
Calculate a value for the Arrhenius constant, AAA, for this reaction. Give your answer to 3 significant figures and include the appropriate units.