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Chapter 12: Problem 81

Assuming that the mechanism for the hydrogenation of $\mathrm{C}_{2} \mathrm{H}_{4}$ given in Section 12.7 is correct, would you predict that the product of the reaction of \(\mathrm{C}_{2} \mathrm{H}_{4}\) with \(\mathrm{D}_{2}\) would be $\mathrm{CH}_{2} \mathrm{D}-\mathrm{CH}_{2} \mathrm{D}\( or \)\mathrm{CHD}_{2}-\mathrm{CH}_{3} ?$ How could the reaction of \(\mathrm{C}_{2} \mathrm{H}_{4}\) with \(\mathrm{D}_{2}\) be used to confirm the mechanism for the hydrogenation of \(\mathrm{C}_{2} \mathrm{H}_{4}\) given in Section 12.7\(?\)

Short Answer

Expert verified
Based on the mechanism given in Section 12.7 for the hydrogenation of C2H4, the predicted product of the reaction of C2H4 with D2 would be CH2D-CH2D (C2H4D2). This reaction can be used to confirm the mechanism by comparing the predicted product with the experimentally observed product. If the observed product matches the predicted CH2D-CH2D, it would support the given mechanism. If it differs, further investigation would be needed.

Step by step solution

01

Identify the Mechanism of Hydrogenation of C2H4

To solve this problem, we first need to understand the mechanism of hydrogenation of C2H4. According to Section 12.7, the reaction takes place as follows: 1. The pi bond of C2H4 reacts with one hydrogen of a dihydrogen molecule (H2) to form a C2H5 intermediate. 2. The C2H5 intermediate then reacts with the second hydrogen of the dihydrogen molecule, resulting in the final product, C2H6 (Ethane).
02

Predict the Product of Reaction of C2H4 with D2

Now, we need to use a similar reasoning to predict the product of the reaction between C2H4 and D2. We follow the mechanism that has been given for the hydrogenation of C2H4: 1. The pi bond of C2H4 reacts with one deuterium (D) of D2 to form a C2H4D intermediate. 2. The C2H4D intermediate reacts with the second deuterium of the D2 molecule. The predicted product would be CH2D-CH2D (C2H4D2).
03

Use the Reaction to Confirm the Mechanism

The reaction of C2H4 with D2 can be used to confirm the mechanism provided in Section 12.7 by observing the product obtained experimentally. If the product is CH2D-CH2D as predicted, it would support the mechanism given in Section 12.7 because the reaction followed the same pathway as the hydrogenation of C2H4. If the experimental product is different, such as CHD2-CH3, it would suggest that the mechanism for the hydrogenation of C2H4 may not be entirely correct, and further investigation would be needed.

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Most popular questions from this chapter

Which of the following statement(s) is(are) true? a. The half-life for a zero-order reaction increases as the reaction proceeds. b. A catalyst does not change the value of \(\Delta \mathrm{E}\) . c. The half-life for a reaction, aA \(\longrightarrow\) products, that is first order in A increases with increasing \([\mathrm{A}]_{0} .\) d. The half-life for a second-order reaction increases as the reaction proceeds.

The mechanism for the gas-phase reaction of nitrogen dioxide with carbon monoxide to form nitric oxide and carbon dioxide is thought to be $$ \begin{array}{c}{\mathrm{NO}_{2}+\mathrm{NO}_{2} \longrightarrow \mathrm{NO}_{3}+\mathrm{NO}} \\ {\mathrm{NO}_{3}+\mathrm{CO} \longrightarrow \mathrm{NO}_{2}+\mathrm{CO}_{2}}\end{array} $$ Write the rate law expected for this mechanism. What is the overall balanced equation for the reaction?

The decomposition of iodoethane in the gas phase proceeds according to the following equation: $$ \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{I}(g) \longrightarrow \mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{H}(g) $$ At \(660 . \mathrm{K}, k=7.2 \times 10^{-4} \mathrm{s}^{-1} ;\) at $720 . \mathrm{K}, k=1.7 \times 10^{-2} \mathrm{s}^{-1}$ What is the value of the rate constant for this first-order decomposition at \(325^{\circ} \mathrm{C} ?\) If the initial pressure of iodoethane is 894 torr at \(245^{\circ} \mathrm{C},\) what is the pressure of iodoethane after three half-lives?

Sulfuryl chloride undergoes first-order decomposition at $320 .^{\circ} \mathrm{C}\( with a half-life of 8.75 \)\mathrm{h}$ . $$ \mathrm{SO}_{2} \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{SO}_{2}(g)+\mathrm{Cl}_{2}(g) $$ What is the value of the rate constant, \(k,\) in \(\mathrm{s}^{-1}\) ? If the initial pressure of \(\mathrm{SO}_{2} \mathrm{Cl}_{2}\) is 791 torr and the decomposition occurs in a \(1.25-\mathrm{L}\) container, how many molecules of \(\mathrm{SO}_{2} \mathrm{Cl}_{2}\) remain after 12.5 \(\mathrm{h}\) ?

A certain first-order reaction is 45.0\(\%\) complete in 65 s. What are the values of the rate constant and the half-life for this process?
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