Consider the following reaction CH3X Y CH3Y
Consider the following reaction: CH3X + Y → CH3Y + X At 25oC the following two experiments were run, yielding the following data:
Experiment 1: [Y]0 = 3.0 M
Experiment 2: [Y] 0 = 4.5 M
Experiments were also run at 85oC. The value of the rate constant at 85oC was found to be 7.88 × 108 (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 this reaction at 25oC.
b. Determine the half- life at 85oC.
c. Determine Ea for the reaction.
d. Given that the C–X bond energy is known to be about 325 kJ/ mol, suggest a mechanism that explains the results in parts a and c.
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