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Chapter 11: Problem 11

As a metal such as lead melts, what happens to (a) the average kinetic energy of the atoms and (b) the average distance between the atoms?

Short Answer

Expert verified
During the melting process of a metal like lead, (a) the average kinetic energy of the atoms increases as the absorbed heat raises the metal's temperature, and (b) the average distance between atoms increases as the metal transitions from a close-packed solid lattice to a more disordered liquid state.

Step by step solution

01

Understand the melting process

When a metal goes from a solid to a liquid state, it undergoes a phase change called melting. During this process, the metal absorbs heat which results in increased kinetic energy and potential energy of the atoms.
02

Analyze the average kinetic energy during melting

The average kinetic energy of the atoms is dependent on the temperature of the metal. When heat is absorbed during the melting process, the temperature of the metal increases, and so does the average kinetic energy of its atoms. So, during melting, the average kinetic energy of the atoms increases.
03

Analyze the average distance between atoms during melting

In the solid phase, metal atoms are arranged in a close-packed structure with relatively small distances between the atoms. When the metal melts, the structure changes from a solid lattice to a disordered liquid, where the atoms have a higher degree of freedom. This leads to an increase in the average distance between the atoms as they are no longer confined to the regular structure of the solid lattice.
04

Summarize the findings

During the melting process of a metal such as lead, (a) the average kinetic energy of the atoms increases due to the absorbed heat, which raises the temperature of the metal, and (b) the average distance between the atoms increases as the metal undergoes a phase change from a close-packed solid lattice to a more disordered liquid state.

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Most popular questions from this chapter

A watch with a liquid crystal display (LCD) does not function properly when it is exposed to low temperatures during a trip to Antarctica. Explain why the LCD might not function well at low temperature.

Appendix \(\mathrm{B}\) lists the vapor pressure of water at various external pressures. (a) Plot the data in Appendix B, vaporpressure (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 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?

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You are high up in the mountains and boil water to make some tea. However, when you drink your tea, it is not as hot as it should be. You try again and again, but the water is just not hot enough to make a hot cup of tea. Which is the best explanation for this result? (a) High in the mountains, it is probably very dry, and so the water is rapidly evaporating from your cup and cooling it. (b) High in the mountains, it is probably very windy, and so the water is rapidly evaporating from your cup and cooling it. (c) High in the mountains, the air pressure is significantly less than 1 atm, so the boiling point of water is much lower than at sea level. (d) High in the mountains, the air pressure is significantly less than 1 atm, so the boiling point of water is much higher than at sea level.

Indicate whether each statement is true or false: (a) The critical pressure of a substance is the pressure at which it turns into a solid at room temperature. (b) The critical temperature of a substance is the highest temperature at which the liquid phase can form. (c) Generally speaking, the higher the critical temperature of a substance, the lower its critical pressure. (\boldsymbol{d} ) In general the more intermolecular forces there are in a substance, the higher its critical temperature and pressure.
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