Question

Using the reaction mechanism below, answer the following questions: 1. Cl2 -> 2Cl 2. Cl + CHCl3 -> HCl + CCl3 3. Cl + CCl3 -> CCl4 a. What is the chemical equation for the overall reaction? b. If the first step was the slowest step, what is the rate law for the overall reaction? What is the overall order of the reaction? c. If the second step was the slowest step, what is the rate law for the overall reaction? What is the overall order of the reaction? d. How could you test which of the two rate laws is correct? e. Are there any intermediates in the reaction? If so, identify them.

Answer 1

a)     chemical equation for the overall reaction

Cl2 + CHCl3 -----------------> CCl4

b) If the first step was the slowest step,

Rare = K[Cl₂] thus= first   order

c) If the second step was the slowest step

Rare = K[Cl] [CHCl3]                 thus=second order

d) it rate increases with increase in     CHCl3   then                  Rare = K[Cl] [CHCl3]    is correct

it rate increases with increase in   Cl2 but not with CHCl3   then    Rare = K[Cl]    is correct

e)   yes         CCl3 and    Cl