1. The problem statement, all variables and given/known data 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!