Question

The dimerization of butadiene 2C4H61 g2h C8H121 g2 was studied at 500. K, and the following data were obtained: Time (s) [C4H6] (mol/L) 195 1.6 3 1022 604 1.5 3 1022 1246 1.3 3 1022 2180 1.1 3 1022 6210 0.68 3 1022 Assuming that Rate 52 D3C4H64 Dt determine the form of the rate law, the integrated rate law, and the value of the rate constant for this reaction.

Answer 1

Answer:

Rate law: $k[C_4H_6]^2$

Integrated Rate Law: $\frac{1}{[C_4H_6]}=\frac{1}{[C_4H_6]_0}+kt$

$k = 1.4 \times 10^{-2}$

Explanation:

We can see that the graph of time is linear compared to $\frac{1}{[C_4H_6]}$ and the reaction is second order hence we get the rate law from $k[A]^n$.

The integrated rate law for second order is $\frac{1}{[A]}=\frac{1}{[A]_0} +kt$ where A is $C_4H_6$.

The slope of the graph $\frac{1}{[C_4H_6]}$ w.r.t time is equal to k. The slope of the graph from the table is 0.014 which is equal to k.