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.

Question

Rosemary Norris

Chemistry

14 September, 09:52

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.

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Monique Spencer · Answer 1

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.