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Chapter 13: Problem 50

Reactions can be classified as unimolecular, bimolecular, and so on. Why are there no zeromolecular reactions? Explain why termolecular reactions are rare.

Short Answer

Expert verified
There are no zeromolecular reactions because chemical reactions, by definition, involve the rearrangement of atoms among molecules. Termolecular reactions, which involve three separate molecules colliding at the same time and in the correct orientation, are rare due to their low probability.

Step by step solution

01

Defining Reactions based on Molecular Concentration

First, it's important to understand what is meant by unimolecular, bimolecular, and termolecular reactions. Unimolecular reactions are reactions that involve only one molecule. Bimolecular reactions involve two molecules. Termolecular reactions involve three molecules.
02

Zeromolecular Reactions

A zeromolecular reaction would theoretically involve zero reacting molecules. Since chemical reactions, by definition, involve the rearrangement of atoms among molecules, there can be no zeromolecular reactions. Without molecules, there would be no reaction.
03

Termolecular Reactions

Termolecular reactions, involving three separate molecules, are relatively rare. This is due to the low probability of three separate molecules colliding at the same time and in the correct orientation to undergo a reaction. The kinetic energy and specific alignment that would be needed make these reactions infrequent in contrast to unimolecular and bimolecular reactions.

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Most popular questions from this chapter

Determine the molecularity and write the rate law for each of the following elementary steps: (a) \(\mathrm{X} \longrightarrow\) products (b) \(\mathrm{X}+\mathrm{Y} \longrightarrow\) products (c) \(\mathrm{X}+\mathrm{Y}+\mathrm{Z} \longrightarrow\) products (d) \(\mathrm{X}+\mathrm{X} \longrightarrow\) products (e) \(\mathrm{X}+2 \mathrm{Y} \longrightarrow\) products

Consider the zero-order reaction: \(\mathrm{A} \longrightarrow\) product. (a) Write the rate law for the reaction. (b) What are the units for the rate constant? (c) Plot the rate of the reaction versus [A].

The equation for the combustion of ethane \(\left(\mathrm{C}_{2} \mathrm{H}_{6}\right)\) is $$ 2 \mathrm{C}_{2} \mathrm{H}_{6}(g)+7 \mathrm{O}_{2}(g) \longrightarrow 4 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) $$ Explain why it is unlikely that this equation also represents the elementary step for the reaction.

Consider the reaction $$ \mathrm{A}+\mathrm{B} \longrightarrow \text { products } $$ From the following data obtained at a certain temperature, determine the order of the reaction and calculate the rate constant. $$ \begin{array}{ccc} \hline[\mathrm{A}](M) & {[\mathrm{B}](M)} & \text { Rate }(M / \mathrm{s}) \\ \hline 1.50 & 1.50 & 3.20 \times 10^{-1} \\ 1.50 & 2.50 & 3.20 \times 10^{-1} \\ 3.00 & 1.50 & 6.40 \times 10^{-1} \\ \hline \end{array} $$

A certain reaction is known to proceed slowly at room temperature. Is it possible to make the reaction proceed at a faster rate without changing the temperature?
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