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Chapter 15: Problem 3

Briefly describe the importance of equilibrium in the study of chemical reactions.

Short Answer

Expert verified
Equilibrium in chemistry refers to the state when rates of forward and reverse reactions are equal, leading to no overall net effect. It's crucial in studying chemical reactions because it lets us predict the concentration of reactants and products at any point in a reaction, allowing us to manipulate a reaction's conditions to get a desired result. In addition, it helps us understand why some reactions do not go to completion, and an equilibrium state still exists.

Step by step solution

01

Define Equilibrium

In the context of chemistry, equilibrium refers to the state where the forward and reverse reactions occur at the same rate, leading to no overall net effect. It does not necessarily mean that the reactants and products are equal in quantity, but that their ratios stay constant.
02

Explain the Occurrence of Equilibrium in Reactions

Equilibrium occurs in a chemical reaction when the rate of reaction in forward direction equals the rate of reverse reaction. It means that the reactants react to form the products, and the products decompose to form the reactants at the same rate.
03

Discuss the Importance of Equilibrium in the Study of Chemical Reactions

Understanding equilibrium is essential in the study of chemical reactions because it allows us to predict the concentrations of reactants and products at any given time in a reaction. This understanding can be used to manipulate conditions of a reaction to get the desired result. For example, to maximise product output in industrial reactions. Additionally, some reactions do not go to completion, and equilibrium will still exist 鈥� an understanding of that allows us to make sense of why that happens.

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Most popular questions from this chapter

Eggshells are composed mostly of calcium carbonate \(\left(\mathrm{CaCO}_{3}\right)\) formed by the reaction $$ \mathrm{Ca}^{2+}(a q)+\mathrm{CO}_{3}^{2-}(a q) \rightleftharpoons \mathrm{CaCO}_{3}(s) $$ The carbonate ions are supplied by carbon dioxide produced as a result of metabolism. Explain why eggshells are thinner in the summer, when the rate of chicken panting is greater. Suggest a remedy for this situation.

Consider the following equilibrium process at \(700^{\circ} \mathrm{C}\) $$ 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g) \rightleftharpoons 2 \mathrm{H}_{2} \mathrm{~S}(g) $$ Analysis shows that there are 2.50 moles of \(\mathrm{H}_{2}, 1.35 \times\) \(10^{-5}\) mole of \(\mathrm{S}_{2}\), and 8.70 moles of \(\mathrm{H}_{2} \mathrm{~S}\) present in a 12.0-L flask at equilibrium. Calculate the equilibrium constant \(K_{\mathrm{c}}\) for the reaction.

Consider the following reaction at \(1600^{\circ} \mathrm{C}\) : $$ \mathrm{Br}_{2}(g) \rightleftharpoons 2 \mathrm{Br}(g) $$ When 1.05 moles of \(\mathrm{Br}_{2}\) are put in a 0.980 - \(\mathrm{L}\) flask, 1.20 percent of the \(\mathrm{Br}_{2}\) undergoes dissociation. Calculate the equilibrium constant \(K_{\mathrm{c}}\) for the reaction.

Write the equilibrium constant expressions for \(K_{\mathrm{c}}\) and \(K_{P}\), if applicable, for these reactions: (a) \(2 \mathrm{NO}_{2}(g)+7 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)+4 \mathrm{H}_{2} \mathrm{O}(l)\) (b) \(2 \mathrm{ZnS}(s)+3 \mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{ZnO}(s)+2 \mathrm{SO}_{2}(g)\) (c) \(\mathrm{C}(s)+\mathrm{CO}_{2}(g) \rightleftharpoons 2 \mathrm{CO}(g)\) (d) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}(a q) \rightleftharpoons \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COO}^{-}(a q)+\mathrm{H}^{+}(a q)\)

The equilibrium constant \(K_{P}\) for the following reaction is found to be \(4.31 \times 10^{-4}\) at \(375^{\circ} \mathrm{C}\) : $$ \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g) $$ In a certain experiment a student starts with 0.862 atm of \(\mathrm{N}_{2}\) and 0.373 atm of \(\mathrm{H}_{2}\) in a constant-volume vessel at \(375^{\circ} \mathrm{C}\). Calculate the partial pressures of all species when equilibrium is reached.
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