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Chapter 12: Problem 71

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
The product of the reaction between \(\mathrm{C}_{2}\mathrm{H}_{4}\) and \(\mathrm{D}_{2}\) would be \(\mathrm{CH}_{2}\mathrm{D}-\mathrm{CH}_{2}\mathrm{D}\), based on the hydrogenation mechanism given in Section 12.7. The reaction can confirm the mechanism, as the formation of this product is consistent with the transfer of deuterium atoms to the double-bonded carbon atoms in the ethene molecule.

Step by step solution

01

Write down the mechanism

The reaction mechanism for the hydrogenation of ethene (\(\mathrm{C}_{2}\mathrm{H}_{4}\)) involves the formation of a pi complex between ethene and the hydrogen molecule, followed by the transfer of hydrogen atoms to the double-bonded carbon atoms, leading to the formation of ethane. In this case, we will consider the same mechanism with deuterium (\(\mathrm{D}_{2}\)) instead of hydrogen.
02

Apply the mechanism to the given reaction

Using the known mechanism, let's apply it to the reaction between \(\mathrm{C}_{2}\mathrm{H}_{4}\) and \(\mathrm{D}_{2}\). In the first step, a pi complex forms between the ethene molecule and the deuterium molecule. In the second step, the deuterium atoms will transfer to the ethene molecule.
03

Determine the product

According to the known mechanism, both deuterium atoms will transfer to the double-bonded carbon atoms in the ethene molecule, leading to the formation of \(\mathrm{CH}_{2}\mathrm{D}-\mathrm{CH}_{2}\mathrm{D}\) as the major product.
04

Discuss the mechanism confirmation

If the reaction between \(\mathrm{C}_{2}\mathrm{H}_{4}\) and \(\mathrm{D}_{2}\) yields a major product of \(\mathrm{CH}_{2}\mathrm{D}-\mathrm{CH}_{2}\mathrm{D}\), it confirms the mechanism for the hydrogenation of \(\mathrm{C}_{2}\mathrm{H}_{4}\). This is because the mechanism involves the transfer of deuterium (or hydrogen) atoms to the double-bonded carbon atoms, and the observed product formation is consistent with this mechanism.

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Most popular questions from this chapter

The type of rate law for a reaction, either the differential rate law or the integrated rate law, is usually determined by which data is easiest to collect. Explain.

The activation energy of a certain uncatalyzed biochemical reaction is \(50.0 \mathrm{~kJ} / \mathrm{mol}\). In the presence of a catalyst at \(37^{\circ} \mathrm{C}\), the rate constant for the reaction increases by a factor of \(2.50 \times 10^{3}\) as compared with the uncatalyzed reaction. Assuming the frequency factor \(A\) is the same for both the catalyzed and uncatalyzed reactions, calculate the activation energy for the catalyzed reaction.

Table \(12.2\) illustrates how the average rate of a reaction decreases with time. Why does the average rate decrease with time? How does the instantaneous rate of a reaction depend on time? Why are initial rates used by convention?

Provide a conceptual rationale for the differences in the half-lives of zero-, first-, and second-order reactions.

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