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Chapter 14: Problem 39

What do we mean by the mechanism of a reaction?

Short Answer

Expert verified
The mechanism of a reaction refers to the sequence of steps that make up the overall reaction, which includes the intermediates, transition states and rate-determining steps. It provides a detailed description of how a chemical reaction takes place.

Step by step solution

01

Define the term 'Mechanism of a Reaction'

A reaction mechanism describes the process by which a chemical reaction takes place. It outlines the individual steps that occur during a reaction, and also defines the intermediates, transition states, and rate-determining steps involved in the reaction.
02

Explain each part of a reaction mechanism

A reaction mechanism has multiple parts to it. Firstly, intermediates are the temporary species that are formed during the reaction, but are not present in the final reaction. Transition states, on the other hand, are the peak-energy states that occur during chemical reactions. Finally, rate-determining steps, which are the slowest steps in a reaction, determine the overall speed or rate of the reaction.
03

Discuss the importance of a reaction mechanism

A reaction mechanism is significant as it allows chemists to understand how a chemical reaction occurs, and this can help to predict the results of similar reactions. It also provides insights into how the reaction can be controlled or manipulated, such as by changing the temperature or using a catalyst to speed up the reaction.

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Most popular questions from this chapter

Write the reaction rate expressions for these reactions in terms of the disappearance of the reactants and the appearance of products: (a) \(\mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \longrightarrow 2 \mathrm{HI}(g)\) (b) \(2 \mathrm{H}_{2}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(g)\) (c) \(5 \mathrm{Br}^{-}(a q)+\mathrm{BrO}_{3}^{-}(a q)+6 \mathrm{H}^{+}(a q) \longrightarrow\) $$ 3 \mathrm{Br}_{2}(a q)+3 \mathrm{H}_{2} \mathrm{O}(l) $$

For the reaction \(X_{2}+Y+Z \longrightarrow X Y+X Z\) it is found that doubling the concentration of \(\mathrm{X}_{2}\) doubles the reaction rate, tripling the concentration of \(Y\) triples the rate, and doubling the concentration of \(Z\) has no effect. (a) What is the rate law for this reaction? (b) Why is it that the change in the concentration of \(Z\) has no effect on the rate? (c) Suggest a mechanism for the reaction that is consistent with the rate law.

The rate constant of a first-order reaction is \(66 \mathrm{~s}^{-1}\) What is the rate constant in units of minutes?

For each of these pairs of reaction conditions, indicate which has the faster rate of formation of hydrogen gas: (a) sodium or potassium with water, (b) magnesium or iron with \(1.0 \mathrm{M} \mathrm{HCl}\), (c) magnesium rod or magnesium powder with \(1.0 \mathrm{M} \mathrm{HCl}\), (d) magnesium with \(0.10 M \mathrm{HCl}\) or magnesium with \(1.0 \mathrm{M} \mathrm{HCl}\).

The rate constant for the second-order reaction $$ 2 \mathrm{NOBr}(g) \longrightarrow 2 \mathrm{NO}(g)+\mathrm{Br}_{2}(g) $$ is \(0.80 / M \cdot \mathrm{s}\) at \(10^{\circ} \mathrm{C}\). (a) Starting with a concentration of \(0.086 M,\) calculate the concentration of \(\mathrm{NOBr}\) after \(22 \mathrm{~s}\) (b) Calculate the half-lives when \([\mathrm{NOBr}]_{0}=\) \(0.072 M\) and \([\mathrm{NOBr}]_{0}=0.054 \mathrm{M}\).
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