Answer to Question #76808 in Physical Chemistry for Tina

Question

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.

Answer 1

Dear Tina, your question requires a lot of work, which neither of our experts is ready to perform for free. We advise you to convert it to a fully qualified order and we will try to help you. Please click the link below to proceed: Submit order