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a) From experimental studies, the reaction: A- B + C is found to be a first-order reaction with rate constant k —— 3.6 x 10-3 s-1at T= 298 K. i) Write down the rate law for the reaction. ii) Calculate the half-life of the reaction at T = 298 K. iii) The activation energy for the reaction is 46.8 kJ mol-1. Assuming that the reaction obeys the Arrhenius Equation, determine the rate constant k for the reaction at T = 320 K. [ R= 8.314 J m )-1 K -1] b) For a reaction of the following type: X -- Products the concentration of the reactant X (denoted [X]) was measured as a function of time I at T = 298 K. The measured data are as follows: [1] [2] [5] t I s [X] / mol dm"3 0 10 60 200 500 0.500 0.351 0.145 0.0543 0.0233 Deduce the order of the reaction and determine the value of the rate constant for the reaction at T = 298 K.
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