In your laboratory you\'re studying a chemical reaction that follows the general
ID: 599816 • Letter: I
Question
In your laboratory you're studying a chemical reaction that follows the general rate law: rate = k[A]. Initial experiments show a rate of 0.001412 M/s when [A] = 0.519 M at 299 K. You add a catalyst to the reaction, which is known to change the activation energy of the process by 1.5 kJ. What will the rate of the reaction be with the catalyst when [A] = 0.0757 M at 315 K? Assume that the Arrhenius factor for this reaction has been determined to be 0.673 s-1.Explanation / Answer
K = rate/[A]2 = 0.001412 / 0.519 = 2.72* 10^-3 K = A exp(-Ea / RT) => 2.72* 10^-3 = 0.673 * exp(-Ea / 8.314 *299) => Ea = 13699 J Ea2 = 13699 - 1500 = 12199 J K2 = A exp(-Ea/RT) => K2 = 0.673 * exp(-12199 / 8.314*315) => K2 = 6.38 * 10^-3 => rate = K2[A] = 6.38 *10^-3 * 0.0757^2 = 4.83 * 10^-4 M/s