In your laboratory you're studying a chemical reaction that follows the general rate law: rate = k[A]2. Initial experiments show a rate of 0.0009784 M/s when [A] = 0.871 M at 279 K. You add a catalyst to the reaction, which is known to change the activation energy of the process by 4.3 kJ. What will the rate of the reaction be with the catalyst when [A] = 0.0547 M at 323 K? Assume that the Arrhenius factor for this reaction has been determined to be 0.729 M-1s-1.