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Chapter 12: Problem 1

Define stability from both a kinetic and thermodynamic perspective. Give examples to show the differences in these concepts.

Short Answer

Expert verified
Kinetic stability refers to the rate of reaction, with a kinetically stable substance having a high activation energy barrier, making it difficult for reactants to convert into products. Thermodynamic stability is about the energy difference between reactants and products, with a thermodynamically stable substance having lower energy than its potential products. An example of kinetic stability is the slow conversion of diamond to graphite, while an example of thermodynamic stability is the mixture of hydrogen and oxygen gases at room temperature, which have the potential to form water but do not do so spontaneously. The main difference between kinetic and thermodynamic stability is their focus on the rate of reaction versus energy differences between reactants and products, respectively.

Step by step solution

01

Define kinetic stability

Kinetic stability refers to the rate of reaction or the speed at which a chemical species converts into another. A chemically stable substance is kinetically stable if the conversion to other products takes a longer time. This means that the reaction has a high activation energy barrier, making it difficult for the reactants to convert into products.
02

Define thermodynamic stability

Thermodynamic stability refers to the difference in energy between the reactants and products of a reaction. A chemically stable substance is thermodynamically stable if its energy is lower than its potential products. This means that the reaction is energetically unfavorable, and a spontaneous conversion to other products is unlikely to occur.
03

Provide an example for kinetic stability

An example of kinetic stability is the stability of diamond. Diamonds are kinetically stable because they have a high activation energy barrier for conversion to graphite. This means that the conversion of diamond to graphite occurs very slowly, even though, thermodynamically, graphite is more stable than diamond.
04

Provide an example for thermodynamic stability

An example of thermodynamic stability can be observed in the reaction between hydrogen and oxygen gases. When mixed together at room temperature, hydrogen and oxygen are thermodynamically unstable; they have the potential to form water, a more stable product. However, this reaction does not occur spontaneously at room temperature because of kinetic stability. The energy barrier required to initiate the reaction is too high, so the reaction is slow.
05

Highlight the differences between kinetic and thermodynamic stability

The primary difference between kinetic and thermodynamic stability is that kinetic stability is focused on the rate of reaction (how fast a reaction can occur), while thermodynamic stability is concerned with the overall energy differences between reactants and products. A substance can be kinetically stable but thermodynamically unstable, meaning it does not react spontaneously but can still form more stable products given enough time or energy input. In contrast, a substance can also be thermodynamically stable and kinetically unstable, meaning it has the potential to form less stable products quickly, but it does not do so because the energy barrier is too high.

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Most popular questions from this chapter

At \(40^{\circ} \mathrm{C}, \mathrm{H}_{2} \mathrm{O}_{2}(a q)\) will decompose according to the following reaction: $$ 2 \mathrm{H}_{2} \mathrm{O}_{2}(a q) \longrightarrow 2 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(\mathrm{~g}) $$ The following data were collected for the concentration of \(\mathrm{H}_{2} \mathrm{O}_{2}\) at various times. $$ \begin{array}{|cc|} \hline \begin{array}{c} \text { Time } \\ (\mathbf{s}) \end{array} & \begin{array}{c} {\left[\mathrm{H}_{2} \mathrm{O}_{2}\right]} \\ (\mathrm{mol} / \mathrm{L}) \end{array} \\ \hline 0 & 1.000 \\ \hline 2.16 \times 10^{4} & 0.500 \\ \hline 4.32 \times 10^{4} & 0.250 \\ \hline \end{array} $$ a. Calculate the average rate of decomposition of \(\mathrm{H}_{2} \mathrm{O}_{2}\) between 0 and \(2.16 \times 10^{4} \mathrm{~s}\). Use this rate to calculate the average rate of production of \(\mathrm{O}_{2}(g)\) over the same time period. b. What are these rates for the time period \(2.16 \times 10^{4} \mathrm{~s}\) to \(4.32 \times 10^{4} \mathrm{~s} ?\)

The reaction $$ 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g) $$ exhibits the rate law $$ \text {Rate} =k[\mathrm{NO}]^{2}\left[\mathrm{O}_{2}\right] $$ Which of the following mechanisms is consistent with this rate law? $$ \begin{array}{l}{\text { a. } \mathrm{NO}+\mathrm{O}_{2} \longrightarrow \mathrm{NO}_{2}+\mathrm{O}} \\ {\mathrm{O}+\mathrm{NO} \longrightarrow \mathrm{NO}_{2}} \\ {\text { b. } \mathrm{NO}+\mathrm{O}_{2} \rightleftharpoons \mathrm{NO}_{3}} \\ {\mathrm{NO}_{3}+\mathrm{NO} \longrightarrow 2 \mathrm{NO}_{2}}\end{array} $$ $$ \begin{array}{l}{\text { c. } 2 \mathrm{NO} \longrightarrow \mathrm{N}_{2} \mathrm{O}_{2}} \\ {\mathrm{N}_{2} \mathrm{O}_{2}+\mathrm{O}_{2} \longrightarrow \mathrm{N}_{2} \mathrm{O}_{4}} \\ {\mathrm{N}_{2} \mathrm{O}_{4} \longrightarrow 2 \mathrm{NO}_{2}} \\ {\text { d. } 2 \mathrm{NO} \rightleftharpoons \mathrm{N}_{2} \mathrm{O}_{2}} \\\ {\mathrm{N}_{2} \mathrm{O}_{2} \longrightarrow \mathrm{NO}_{2}+\mathrm{O}} \\\ {\mathrm{O}+\mathrm{NO} \longrightarrow \mathrm{NO}_{2}}\end{array} $$

Each of the statements given below is false. Explain why. a. The activation energy of a reaction depends on the overall energy change \((\Delta E)\) for the reaction. b. The rate law for a reaction can be deduced from examination of the overall balanced equation for the reaction. c. Most reactions occur by one-step mechanisms.

The decomposition of \(\mathrm{NO}_{2}(g)\) occurs by the following bimolecular elementary reaction: $$ 2 \mathrm{NO}_{2}(g) \longrightarrow 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) $$ The rate constant at 273 \(\mathrm{K}\) is \(2.3 \times 10^{-12} \mathrm{L} / \mathrm{mol} \cdot \mathrm{s}\) , and the activation energy is 111 \(\mathrm{kJ} / \mathrm{mol}\) . How long will it take for the concentration of \(\mathrm{NO}_{2}(g)\) to decrease from an initial partial pressure of 2.5 \(\mathrm{atm}\) to 1.5 \(\mathrm{atm}\) at \(500 . \mathrm{K}\) ? Assume ideal gas behavior.

The activation energy for some reaction $$ \mathrm{X}_{2}(g)+\mathrm{Y}_{2}(g) \longrightarrow 2 \mathrm{XY}(g) $$ is 167 \(\mathrm{kJ} / \mathrm{mol}\) , and \(\Delta E\) for the reaction is \(+28 \mathrm{kJ} / \mathrm{mol}\) . What is the activation energy for the decomposition of XY?
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