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Chapter 11: Problem 10

(a) How does the average kinetic energy of molecules compare with the average energy of attraction between molecules in solids, liquids, and gases? (b) Why does increasing the temperature cause a solid substance to change in succession from a solid to a liquid to a gas? (c) What happens to a gas if you put it under extremely high pressure?

Short Answer

Expert verified
(a) In solids, the kinetic energy of molecules is relatively low, and the intermolecular attraction energy is high. In liquids, the kinetic energy is higher than in solids, and the intermolecular attraction energy is less than in solids but still significant. In gases, the kinetic energy is the highest, and the intermolecular attraction energy is the weakest or almost negligible. (b) When the temperature of a solid substance is increased, the average kinetic energy of particles increases, causing the substance to change from solid to liquid at the melting point and liquid to gas at the boiling point. (c) When a gas is subjected to extremely high pressure, the particles are forced closer together, and the volume decreases, causing the gas to transform into a liquid or a solid through compression.

Step by step solution

01

(a) Comparing kinetic energy and intermolecular attraction energy in solids, liquids, and gases

In solids, the atoms or molecules are closely packed together and have a definite shape and volume. The kinetic energy of molecules in solids is relatively low, while the intermolecular attraction energy is high. In liquids, atoms or molecules are loosely packed and have no definite shape, but they have a definite volume. In this case, the average kinetic energy is higher than in solids, and the intermolecular attraction energy is less than in solids but still significant enough to keep the particles together. In gases, atoms or molecules are far apart, with no definite shape and volume. The average kinetic energy in gases is the highest among all three states of matter, while the intermolecular attraction energy is the weakest or almost negligible.
02

(b) Effects of increasing temperature on a solid substance

When the temperature of a solid substance is increased, the average kinetic energy of the particles also increases. 1. Solid to Liquid - When the energy added is sufficient to overcome the intermolecular attraction, the solid substance starts to melt, changing into a liquid state. The melting point is the temperature at which the solid turns into a liquid. 2. Liquid to Gas - As the temperature continues to increase and the kinetic energy of the particles becomes greater, the intermolecular attraction further weakens. Once the energy is enough to completely overcome the intermolecular attraction between the particles, the substance starts to boil and transform from a liquid to a gaseous state. The boiling point is the temperature at which the liquid turns into a gas.
03

(c) Effects of high pressure on a gas

When a gas is subjected to extremely high pressure, the particles are forced closer together, and the volume decreases. Due to the increased proximity of particles, the intermolecular attraction forces start playing a more significant role. As a result, the gas may combine to form a liquid or even a solid, depending on the nature of the substance and the applied pressure. This process of transforming a gas into a liquid or a solid due to high pressure is known as compression.

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Most popular questions from this chapter

The relative humidity of air equals the ratio of the partial pressure of water in the air to the equilibrium vapor pressure of water at the same temperature times \(100 \% .\) If the relative humidity of the air is \(58 \%\) and its temperature is \(68^{\circ} \mathrm{F}\), how many molecules of water are present in a room measuring \(12 \mathrm{ft} \times 10 \mathrm{ft} \times 8 \mathrm{ft} ?\)

Name the phase transition in each of the following situations and indicate whether it is exothermic or endothermic: (a) When ice is heated, it turns to water. (b) Wet clothes dry on a warm summer day. (c) Frost appears on a window on a cold winter day. (d) Droplets of water appear on a cold glass of beer.

Appendix B lists the vapor pressure of water at various external pressures. (a) Plot the data in Appendix B, vapor pressure (torr) versus temperature \(\left({ }^{\circ} \mathrm{C}\right) .\) From your plot, estimate the vapor pressure of water at body temperature, \(37^{\circ} \mathrm{C}\). (b) Explain the significance of the data point at 760.0 torr, \(100^{\circ} \mathrm{C}\) (c) A city at an altitude of \(5000 \mathrm{ft}\) above sea level has a barometric pressure of 633 torr. To what temperature would you have to heat water to boil it in this city? (d) A city at an altitude of \(500 \mathrm{ft}\) below sea level would have a barometric pressure of 774 torr. To what temperature would you have to heat water to boil it in this city? (e) For the two cities in parts \((\mathrm{c})\) and \((\mathrm{d}),\) compare the average kinetic energies of the water molecules at their boiling points. Are the kinetic energies the same or different? Explain.

The fact that water on Earth can readily be found in all three states (solid, liquid, and gas) is in part a consequence of the fact that the triple point of water \(\left(T=0.01^{\circ} \mathrm{C}, P=0.006 \mathrm{~atm}\right)\) falls within a range of temperatures and pressures found on Earth. Saturn's largest moon Titan has a considerable amount of methane in its atmosphere. The conditions on the surface of Titan are estimated to be \(P=1.6\) atm and \(T=-178^{\circ} \mathrm{C}\). As seen from the phase diagram of methane (Figure 11.30 ), these conditions are not far from the triple point of methane, raising the tantalizing possibility that solid, liquid, and gaseous methane can be found on Titan. (a) What state would you expect to find methane in on the surface of Titan? (b) On moving upward through the atmosphere the pressure will decrease. If we assume that the temperature does not change, what phase change would you expect to see as we move away from the surface?

Look up and compare the normal boiling points and normal melting points of \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{H}_{2} \mathrm{~S}\). Based on these physical properties, which substance has stronger intermolecular forces? What kinds of intermolecular forces exist for each molecule?
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