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Chapter 9: Problem 17

Use the kinetic molecular theory to explain why a liquid gets cooler as it evaporates from an insulated container.

Short Answer

Expert verified
In summary, evaporation cools a liquid in an insulated container because higher-energy particles escape during evaporation, leaving behind lower-energy particles. This causes the average kinetic energy, and therefore the temperature, to decrease. The insulated container prevents heat exchange with the surroundings, making the cooling effect more noticeable.

Step by step solution

01

Understanding Kinetic Molecular Theory

The kinetic molecular theory states that the particles of matter (atoms or molecules) are always in motion and have kinetic energy. In a liquid, these particles are in constant random motion, colliding with each other and with the walls of the container. The kinetic energy of the particles depends on the temperature of the liquid. As the temperature of the liquid increases, the particles move faster and have higher kinetic energy.
02

Evaporation Process

Evaporation is the process in which the liquid particles at the surface gain enough kinetic energy to overcome the attractive forces between them and escape into the vapor phase. The particles with higher kinetic energy are more likely to evaporate since they have a higher probability of obtaining the required energy to break free from the intermolecular forces holding them together.
03

Energy Transfer During Evaporation

When particles with higher kinetic energy escape from the liquid surface during evaporation, they take their energy with them. This leaves behind lower-energy particles in the liquid. As a result, the average kinetic energy of the remaining particles decreases. According to the kinetic molecular theory, a decrease in the average kinetic energy corresponds to a decrease in temperature.
04

Insulated Container's Role

The role of the insulated container is to prevent heat exchange with the surrounding environment. This means that the energy lost during evaporation is not replenished by the transfer of heat from the surroundings, forcing the remaining liquid to experience cooling due to the loss of higher-energy particles.
05

Explaining the Cooling Effect

To sum up, a liquid gets cooler as it evaporates from an insulated container because the particles with higher kinetic energy escape during the process of evaporation, leaving behind lower-energy particles. This results in a decrease in the average kinetic energy of the remaining particles, which corresponds to a decrease in temperature. As the insulated container prevents heat exchange with the surroundings, the liquid's cooling effect is observed.

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Most popular questions from this chapter

Which of the following statements about intermolecular forces is(are) true? a. London dispersion forces are the only type of intermolecular force that nonpolar molecules exhibit. b. Molecules that have only London dispersion forces will always be gases at room temperature \(\left(25^{\circ} \mathrm{C}\right).\) c. The hydrogen-bonding forces in \(\mathrm{NH}_{3}\) are stronger than those in \(\mathrm{H}_{2} \mathrm{O}\). d. The molecules in \(\mathrm{SO}_{2}(g)\) exhibit dipole-dipole intermolecular interactions. e. \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{3}\) has stronger London dispersion forces than does \(\mathrm{CH}_{4}.\)

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