Question

Consider the following reaction:
CH3X + Y --> CH3Y + X
At 25 degrees Celcius the following two experiments were run, yielding the following data:

Experiment 1: [Y]0 = 3.0 M
[CH3X] (mol/L) Time (hours)
7.08*10^-3 1.0
4.52*10^-3 1.5
2.23*10^-3 2.3
4.76*10^-4 4.0
8.44*10^-5 5.7
2.75*10^-5 7.0

Experiment 2: [Y]0 = 4.5 M
[CH3X] (mol/L) Time (hours)
4.50*10^-3 0
1.70*10^-3 1.0
4.19*10^-4 2.5
1.11*10^-4 4.0
2.81*10^-5 5.5

Experiments were also run at 85 degrees Celcius. The value of the rate constant at 85 degrees Celcius was found to be 7.88*10^8 (with the time in units of hours), where [CH3X]0=1.0*10^-2 M and [Y]0= 3.0 M.
a) Determine the rate law and the value of k for the reaction at 25 degrees Celcius.
b) Determine the half-life at 85 degrees Celcius.
c) Determine the activation energy (Ea) for the reaction.
d) Given that C-X bond energy is known to be about 320 kJ/mol, suggest a mechanism that explains the results in parts a and c.

Answer 1

Nice try