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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ICHme (h) 7.08 × 10-3 M 4.52 × 10-3 M 2.23 x 10-3 M 4.76 × 10-4 M 8.44 × 10-5 M 2.75 × 10-5 M 1.0 1.5 2.3 4.0 5.7 7.0 Time (h) 4.50 × 10-3 M 1.70 × 10-3 M 4.19 × 10-4 M 1.11 × 10-4M 2.81 × 10-sM 1.0 2.5 4.0 5.5