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Chapter 10: Problem 20

Describe what is meant by a dynamic equilibrium in terms of the vapor pressure of a liquid.

Short Answer

Expert verified
Dynamic equilibrium in terms of vapor pressure is a state in which the rate of evaporation equals the rate of condensation in a closed system containing a liquid and its vapor. In this state, there is a constant exchange of particles between the liquid and the vapor, maintaining a constant vapor pressure while the overall quantities of liquid and vapor remain stable.

Step by step solution

01

1. Define Dynamic Equilibrium

Dynamic equilibrium is a state in which the rate of a forward process is equal to the rate of its reverse process, resulting in no net change in the system. In this state, the system appears to be stable and unmoving, but in reality, the components are continuously and constantly changing.
02

2. Define Vapor Pressure

Vapor pressure is the pressure exerted by a vapor when it is in equilibrium with its liquid phase. It is a measure of the tendency of liquid particles to escape from the liquid surface and become vapor in the atmosphere above the liquid. Vapor pressure depends on two factors: the temperature of the liquid and the nature of the liquid itself.
03

3. Describe the Relationship Between Dynamic Equilibrium and Vapor Pressure

In the context of vapor pressure, dynamic equilibrium is achieved when the rate of evaporation (liquid particles escaping to form vapor) equals the rate of condensation (vapor particles returning to the liquid phase). At this point, there is a constant exchange of particles between the liquid and its vapor, but the overall quantities of liquid and vapor remain constant.
04

4. Discuss Dynamic Equilibrium in a Closed System

Dynamic equilibrium can be observed in a closed system containing a liquid and its vapor. Initially, the liquid particles begin to evaporate, and the vapor particles rise above the liquid surface. As the vapor pressure above the liquid increases, the rate of condensation also increases. When the rate of evaporation and the rate of condensation become equal, the system reaches dynamic equilibrium. In this state, the vapor pressure remains constant and the system appears stable. However, the individual particles are continuously moving between the liquid and vapor phases.
05

5. Summarize the Concept of Dynamic Equilibrium with Vapor Pressure

In conclusion, dynamic equilibrium in terms of vapor pressure is when the rate of evaporation equals the rate of condensation in the closed system containing a liquid and its vapor. There is a constant exchange of particles between the liquid and the vapor, but the overall quantities of these phases remain stable. This constant exchange of particles maintains a constant vapor pressure in the system.

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Most popular questions from this chapter

An ice cube tray contains enough water at \(22.0{ }^{\circ} \mathrm{C}\) to make 18 ice cubes that each have a mass of \(30.0 \mathrm{~g} .\) The tray is placed in a freezer that uses \(\mathrm{CF}_{2} \mathrm{Cl}_{2}\) as a refrigerant. The heat of vaporization of \(\mathrm{CF}_{2} \mathrm{Cl}_{2}\) is \(158 \mathrm{~J} / \mathrm{g} .\) What mass of \(\mathrm{CF}_{2} \mathrm{Cl}_{2}\) must be vaporized in the refrigeration cycle to convert all the water at \(22.0^{\circ} \mathrm{C}\) to ice at \(-5.0^{\circ} \mathrm{C}\) ? The heat capacities for \(\mathrm{H}_{2} \mathrm{O}(s)\) and \(\mathrm{H}_{2} \mathrm{O}(I)\) are \(2.03 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}\) and \(4.18 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}\), respectively, and the enthalpy of fusion for ice is \(6.02 \mathrm{~kJ} / \mathrm{mol}\).

Superalloys have been made of nickel and aluminum. The alloy owes its strength to the formation of an ordered phase, called the gamma-prime phase, in which Al atoms are at the corners of a cubic unit cell and Ni atoms are at the face centers. What is the composition (relative numbers of atoms) for this phase of the nickel-aluminum superalloy?

Define critical temperature and critical pressure. In terms of the kinetic molecular theory, why is it impossible for a substance to exist as a liquid above its critical temperature?

A plot of \(\ln \left(P_{\text {vap }}\right)\) versus \(1 / T(\mathrm{~K})\) is linear with a negative slope. Why is this the case?

The molar enthalpy of vaporization of water at \(373 \mathrm{~K}\) and \(1.00\) atm is \(40.7 \mathrm{~kJ} / \mathrm{mol}\). What fraction of this energy is used to change the internal energy of the water, and what fraction is used to do work against the atmosphere? (Hint: Assume that water vapor is an ideal gas.)
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