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Chapter 14: Problem 131

In theory, all reactions are reversible, but in practice, some are not. Explain why.

Short Answer

Expert verified
In theory, all reactions are reversible; however, in practice, some reactions are irreversible due to factors such as kinetic factors, thermodynamic factors, side reactions, and product removal. Kinetic factors can make the reverse reaction too slow to be observed, while thermodynamic factors can drive the reaction to completion by releasing a large amount of energy. Side reactions can cause products to undergo additional reactions, making it difficult to revert to the original reactants, and continuous removal of products can prevent the reverse reaction from occurring. Examples of practically irreversible reactions include combustion and precipitation reactions.

Step by step solution

01

Understand reversible and irreversible reactions

In reversible reactions, reactants form products, and products can react with each other to form reactants again. These reactions reach a state of equilibrium, where the rates of the forward reaction (conversion of reactants to products) and the reverse reaction (conversion of products to reactants) become equal. On the other hand, in irreversible reactions, the forward reaction occurs, and the products formed do not revert to the original reactants.
02

Factors contributing to irreversible reactions

There are several factors that lead to some reactions being irreversible, including: 1. Kinetic factors: The reaction rate may be too slow for the reverse reaction to be observed or measured. This makes the reaction seem irreversible. 2. Thermodynamic factors: Some reactions produce a large amount of energy, which drives the reaction to completion, making the reverse reaction less favorable. 3. Side reactions: Some products can undergo side reactions, which makes it difficult for the reaction to go back to the original reactants. 4. Removal of products: If products are removed continuously from the reaction mixture, the reverse reaction is unlikely to occur, and the reaction becomes irreversible.
03

Examples of irreversible reactions

Here are some examples of reactions that are considered irreversible in practice due to the factors mentioned above: 1. Combustion: Burning a fuel, such as methane, in the presence of oxygen is highly exothermic and thermodynamically favored, making the reverse reaction highly unlikely. 2. Precipitation reactions: In reactions where a solid is formed, such as the formation of a salt from a reaction between a metal ion and an anion, the solid formed can be removed, making the reverse reaction practically impossible. In conclusion, while theoretically, all reactions are reversible, several factors make some reactions practically irreversible. Examples include combustion reactions and precipitation reactions.

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Most popular questions from this chapter

Diamond and graphite are two forms of elemental carbon. Under the appropriate conditions they will be in equilibrium with each other: \(C_{\text {diamond }} \rightleftarrows C_{\text {graphite }}\) If graphite is subjected to very high pressure and temperature, it will convert into the diamond form. (a) Is the above equilibrium reaction exothermic or endothermic? Explain how you know. (b) Which form, graphite or diamond, has the higher density? (Hint: Think about what increasing the pressure of a gas does to its density. It works the same for the solid and liquid phases as well.)

Would the solubility of \(\mathrm{PbI}_{2}(s)\) be greater in water or in an aqueous solution of NaI? Explain your answer. (Hint: If \(\left[\mathrm{Pb}^{2+}\right] \times\left[\mathrm{I}^{-}\right]^{2}>K_{\mathrm{sp}}\) ' precipitation will occur.)

Suppose you are making ammonia \(\left(\mathrm{NH}_{3}\right)\) by the Haber reaction, at \(472{ }^{\circ} \mathrm{C}\) : \(3 \mathrm{H}_{2}(g)+\mathrm{N}_{2}(g) \rightleftarrows 2 \mathrm{NH}_{3}(g) K_{\mathrm{eq}}=0.105\) (a) Describe qualitatively where the equilibrium lies for this reaction. (b) On the face of it, would this reaction be a good one for isolating pure ammonia? (c) What would happen if you could keep feeding \(\mathrm{H}_{2}\) and \(\mathrm{N}_{2}\) into the reaction vessel while at the same time removing \(\mathrm{NH}_{3}\) ?

State Le Châtelier's principle using the words undo and partially.

How does decreasing the temperature affect the value of \(K_{e q}\) for an exothermic reaction? (a) Increases \(K_{\text {eq }}\) (b) Decreases \(K_{\text {eq }}\) (c) Does not change \(K_{\text {eq }}\)
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