Question

The unsaturated hydrocarbon butadiene (C4H6) dimerizes to 4-vinylcyclohexan (C8H12).When data collected in studies of the kinetics of this reaction were plotted against reaction time, plots of [C4H6] or ln[C4H6] produced curved lines, but the plot of 1/[C4H6] was linear.a) What is the rate law for the reaction?b) How many half-lives will it take for the [C4H6] to decrease to 3.1% of its original concentration? The relationship of [A]t/[A]o = 0.50^n, where n = the number of half-lives.

Answer 1

Step-by-step explanation:

From the information of the graph plots, the reaction is a second order reaction.

a) What is the rate law for the reaction?

Rate = k [C4H6]²

The superscript 2 signifies it is a second order reaction.

b) How many half-lives will it take for the [C4H6] to decrease to 3.1% of its original concentration?

Using the formular below;

[A]t / [A]o = 0.50^n

[A]t = 100%

[A]o = 3.1%

100 / 3.1 = 0.50^n

32 = 0.50^n

2^5 = 2^-n

n = 5

It would take five half lives.