- #1
annnoyyying
- 44
- 0
Homework Statement
I need help for this kinetics question:
Chlorination of butene at 0 degrees c, liquid phase, dichloromethane as solvent.
initial concentration of butene is 0.1M
conversion of 47.71% achieved after 3.1 hours.
an additional 0.5M of hot butene was added at this point, which increased the temperature of the mixture to 10 degrees c
after another 20mins the concentration of the alkene in the mixture is 0.52M.
Determine the value of the rate constant at 0 degrees C and its temperature dependence.
2. Relevant equation
2nd order integral: 1/[A] = 1/[A]0 +kt
3. The Attempt at a Solution
The reaction will form 1,2 - dichlorobutene due to presence of a non-protic solvent and low reaction temperatures.
I'm guessing the overall order of reaction is 2, mainly because the transition state involves a molecule of chlorine and a molecule of butene. However I do not know the order of reaction in respect to each of the reactants.
For the 1st reaction (at 0 degrees);
concentration of butene at 3.1 hrs is 0.05229 M
reaction rate is 2.565e-4 M/min
As the initial concentrations of both reactants are the same, and using the equation for the 2nd order integral the rate constant at 0 degrees would be 0.0491 L/mol . min.
Then I'm stuck after this. To be honest I'm not even sure if my answers/ logic above is even correct...
Thanks in advance!