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Chapter 14: Problem 1

Define equilibrium. Give two examples of a dynamic equilibrium.

Short Answer

Expert verified
Equilibrium is a state where opposing forces or influences are balanced. A dynamic equilibrium, on the other hand, is when two processes are occurring at the same rate, resulting in no net change. Examples can be the esterification process in chemistry and the phase change between liquid water and steam at boiling point.

Step by step solution

01

Definition

Equilibrium refers to a state in which opposing forces or influences are balanced. In the context of science, it often refers to a state where the rate of change in one direction is the same as the rate of change in the opposite direction, thus resulting in a steady state or a lack of overall change.
02

Example 1 of Dynamic Equilibrium

An example of dynamic equilibrium is a chemical reaction where the rate of formation of products and the rate of formation of reactants both occur simultaneously and at equal speeds. For instance, in the process of esterification, an acid reacts with an alcohol to form an ester and water, this reaction is reversible and can reach a point where both forward and backward reactions are taking place at the same rate.
03

Example 2 of Dynamic Equilibrium

Another example involving dynamic equilibrium is the phase change between liquid water evaporating into steam and steam condensing into liquid water. At the boiling point of water (100 degrees Celsius at standard pressure), liquid water turns into steam at the same rate that steam condenses into liquid water. This allows the amounts of liquid water and steam to remain constant over time, even though individual water molecules continuously change from one phase to another.

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Most popular questions from this chapter

Consider the following reaction at equilibrium: $$\mathrm{A}(g) \rightleftharpoons 2 \mathrm{~B}(g)$$ From the data shown here, calculate the equilibrium constant (both \(K_{P}\) and \(K_{\mathrm{c}}\) ) at each temperature. Is the reaction endothermic or exothermic? $$ \begin{array}{clr} \text { Temperature }\left({ }^{\circ} \mathrm{C}\right) & {[\mathrm{A}](M)} & {[\mathrm{B}](M)} \\ 200 & 0.0125 & 0.843 \\ 300 & 0.171 & 0.764 \\ 400 & 0.250 & 0.724 \end{array} $$

A quantity of 0.20 mole of carbon dioxide was heated to a certain temperature with an excess of graphite in a closed container until the following equilibrium was reached: $$\mathrm{C}(s)+\mathrm{CO}_{2}(g) \rightleftharpoons 2 \mathrm{CO}(g)$$ Under these conditions, the average molar mass of the gases was \(35 \mathrm{~g} / \mathrm{mol}\). (a) Calculate the mole fractions of \(\mathrm{CO}\) and \(\mathrm{CO}_{2}\). (b) What is \(K_{P}\) if the total pressure is 11 atm? (Hint: The average molar mass is the sum of the products of the mole fraction of each gas and its molar mass.

The formation of \(\mathrm{SO}_{3}\) from \(\mathrm{SO}_{2}\) and \(\mathrm{O}_{2}\) is an intermediate step in the manufacture of sulfuric acid, and it is also responsible for the acid rain phenomenon. The equilibrium constant \(K_{P}\) for the reaction $$2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{SO}_{3}(g)$$ is 0.13 at \(830^{\circ} \mathrm{C}\). In one experiment \(2.00 \mathrm{~mol} \mathrm{SO}_{2}\) and \(2.00 \mathrm{~mol} \mathrm{O}_{2}\) were initially present in a flask. What must the total pressure at equilibrium be in order to have an 80.0 percent yield of \(\mathrm{SO}_{3} ?\)

List four factors that can shift the position of an equilibrium. Only one of these factors can alter the value of the equilibrium constant. Which one is it?

A quantity of \(6.75 \mathrm{~g}\) of \(\mathrm{SO}_{2} \mathrm{Cl}_{2}\) was placed in a 2.00-L flask. At \(648 \mathrm{~K}\), there is \(0.0345 \mathrm{~mole}\) of \(\mathrm{SO}_{2}\) present. Calculate \(K_{\mathrm{c}}\) for the reaction $$\mathrm{SO}_{2} \mathrm{Cl}_{2}(g) \rightleftharpoons \mathrm{SO}_{2}(g)+\mathrm{Cl}_{2}(g)$$
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