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Chapter 14: Problem 56

What effect does an increase in pressure have on each of the following systems at equilibrium? The temperature is kept constant and, in each case, the reactants are in a cylinder fitted with a movable piston. (a) \(\mathrm{A}(s) \rightleftharpoons 2 \mathrm{~B}(s)\) (b) \(2 \mathrm{~A}(l) \rightleftharpoons \mathrm{B}(l)\) (c) \(\mathrm{A}(s) \rightleftharpoons \mathrm{B}(g)\) (d) \(\mathrm{A}(g) \rightleftharpoons \mathrm{B}(g)\) (e) \(\mathrm{A}(g) \rightleftharpoons 2 \mathrm{~B}(g)\)

Short Answer

Expert verified
In summary, an increase in pressure does not affect the equilibrium in system (a) and system (b) since solids and liquids do not affect pressure. System (c) will be shifted towards reactant and in system (d), pressure modification does not affect the equilibrium. For system (e), the equilibrium will shift towards the reactant as there are fewer gas molecules on this side.

Step by step solution

01

Exercise (a) Analysis: A(s) ⇌ 2 B(s)

Ensure you understand that solids do not have an effect on pressure. In this reaction, there is no change in the number of moles of the gases. Therefore, changing the pressure does not affect the equilibrium of the reaction.
02

Exercise (b) Analysis: 2 A(l) ⇌ B(l)

Realize that liquids do not have an effect on pressure either. In this reaction, we also see no change in the number of moles of gases. As a result, changing the pressure does not affect the equilibrium of the reaction.
03

Exercise (c) Analysis: A(s) ⇌ B(g)

Keep in mind that solids do not have an effect on pressure. However, this reaction has one mole of gas as product, so an increase in pressure will cause a shift in the equilibrium towards the reactant A to reduce the pressure.
04

Exercise (d) Analysis: A(g) ⇌ B(g)

Pay attention to the number of moles. In this reaction, there is no change in the number of moles of gases. Therefore, changing the pressure does not affect the equilibrium of the reaction.
05

Exercise (e) Analysis: A(g) ⇌ 2 B(g)

Identify the change in the quantity of gas molecules in the system. In this reaction, an increase in pressure will result in a shift in the equilibrium towards the reactant side where there is less number of gas molecules to minimize the pressure.

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Most popular questions from this chapter

Explain the difference between physical equilibrium and chemical equilibrium. Give two examples of each.

The vapor pressure of mercury is \(0.0020 \mathrm{mmHg}\) at \(26^{\circ} \mathrm{C}\). (a) Calculate \(K_{\mathrm{c}}\) and \(K_{P}\) for the process \(\mathrm{Hg}(l) \rightleftharpoons \mathrm{Hg}(g) .\) (b) A chemist breaks a thermometer and spills mercury onto the floor of a laboratory measuring \(6.1 \mathrm{~m}\) long, \(5.3 \mathrm{~m}\) wide, and \(3.1 \mathrm{~m}\) high. Calculate the mass of mercury (in grams) vaporized at equilibrium and the concentration of mercury vapor in \(\mathrm{mg} / \mathrm{m}^{3}\). Does this concentration exceed the safety limit of \(0.05 \mathrm{mg} / \mathrm{m}^{3} ?\) (Ignore the volume of furniture and other objects in the laboratory.)

At room temperature, solid iodine is in equilibrium with its vapor through sublimation and deposition (see Section 11.8). Describe how you would use radioactive iodine, in either solid or vapor form, to show that there is a dynamic equilibrium between these two phases.

Define equilibrium. Give two examples of a dynamic equilibrium.

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? $$ \begin{array}{clr} \text { Temperature }\left({ }^{\circ} \mathrm{C}\right) & {[\mathrm{A}](M)} & {[\mathrm{B}](M)} \\ 200 & 0.0125 & 0.843 \\ 300 & 0.171 & 0.764 \\ 400 & 0.250 & 0.724 \end{array} $$
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