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Chapter 10: 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
During evaporation from an insulated container, high-energy molecules at the liquid's surface escape into the gas phase, taking energy from the remaining liquid. This causes a decrease in the average kinetic energy of the remaining liquid particles and a reduction in the liquid's temperature, resulting in the liquid becoming cooler. This phenomenon can be explained using the kinetic molecular theory, which states that particles in liquids are in constant random motion, exchanging energy through collisions.

Step by step solution

01

Understanding Kinetic Molecular Theory of Liquids

Kinetic molecular theory is a model that describes the behavior of liquids and gases on a molecular level. According to this theory, the particles (atoms or molecules) in liquids are in constant random motion. The motion of these particles makes them collide with one another and with the walls of the container in which the liquid is confined. As a result of these collisions, the particles exchange energy. Some particles will gain energy while others will lose energy.
02

Evaporation Process

Evaporation is the process in which the molecules at the surface of a liquid are converted from the liquid phase to the gas phase. Molecules in a liquid have a range of kinetic energies; some molecules have high energy while others have low energy. When a liquid is exposed to an external environment, the high-energy molecules at the surface have enough energy to escape the liquid phase and enter the gas phase. This process requires energy, which the escaping molecules acquire from the surrounding liquid.
03

Why a Liquid Gets Cooler During Evaporation

When high-energy molecules escape into the gas phase, they take some energy from the remaining liquid. Since this energy is being removed from the liquid, the average kinetic energy of the remaining particles decreases. As a result, the temperature of the liquid drops, and it gets cooler. To summarize, during evaporation from an insulated container, the high-energy molecules at the surface of the liquid escape into the gas phase, taking some energy from the liquid. This results in a decrease in the average kinetic energy of the remaining liquid particles and a drop in the temperature of the liquid, making it cooler.

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Most popular questions from this chapter

Consider the following melting point data: $$ \begin{array}{|llllllll|} \hline \text { Compound: } & \mathrm{NaCl} & \mathrm{MgCl}_{2} & \mathrm{AlCl}_{3} & \mathrm{SiCl}_{4} & \mathrm{PCl}_{3} & \mathrm{SCl}_{2} & \mathrm{Cl}_{2} \\ \operatorname{mp}\left({ }^{\circ} \mathrm{C}\right): & 801 & 708 & 190 & -70 & -91 & -78 & -101 \\ \text { Compound: } & \mathrm{NaF} & \mathrm{MgF}_{2} & \mathrm{AlF}_{3} & \mathrm{SiF}_{4} & \mathrm{PF}_{5} & \mathrm{SF}_{6} & \mathrm{~F}_{2} \\ \operatorname{mp}\left({ }^{\circ} \mathrm{C}\right): & 997 & 1396 & 1040 & -90 & -94 & -56 & -220 \\ \hline \end{array} $$ Account for the trends in melting points in terms of interparticle forces.

Mn crystallizes in the same type of cubic unit cell as Cu. Assuming that the radius of \(\mathrm{Mn}\) is \(5.6 \%\) larger than the radius of \(\mathrm{Cu}\) and the density of copper is \(8.96 \mathrm{~g} / \mathrm{cm}^{3}\), calculate the density of \(\mathrm{Mn}\).

Which are stronger, intermolecular or intramolecular forces for a given molecule? What observation(s) have you made that support this? Explain.

A \(20.0-\mathrm{g}\) sample of ice at \(-10.0^{\circ} \mathrm{C}\) is mixed with \(100.0 \mathrm{~g}\) water at \(80.0^{\circ} \mathrm{C}\). Calculate the final temperature of the mixture assuming no heat loss to the surroundings. The heat capacities of \(\mathrm{H}_{2} \mathrm{O}(s)\) and \(\mathrm{H}_{2} \mathrm{O}(l)\) are \(2.03\) and \(4.18 \mathrm{~J} / \mathrm{g} \cdot{ }^{\circ} \mathrm{C}\), respectively, and the enthalpy of fusion for ice is \(6.02 \mathrm{~kJ} / \mathrm{mol}\).

A substance, \(X\), has the following properties: Sketch a heating curve for substance \(\mathrm{X}\) starting at \(-50 .{ }^{\circ} \mathrm{C}\).
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