Textbook Question
(b) Could you measure the triple point of water by measuring the temperature in a vessel in which water vapor, liquid water, and ice are in equilibrium under 1 atm of air? Explain.
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Ch.11 - Liquids and Intermolecular Forces
Chapter 11, Problem 62a
Use the phase diagram of neon to answer the following questions. (a) What is the approximate value of the normal boiling point?
Verified step by step guidance1
Understand the concept of a phase diagram: A phase diagram is a graphical representation of the physical states of a substance under different conditions of temperature and pressure. It shows the boundaries between different phases (solid, liquid, gas) and the conditions under which these phases coexist in equilibrium.
Identify the 'normal boiling point': The normal boiling point of a substance is the temperature at which it changes from a liquid to a gas at 1 atmosphere (atm) of pressure.
Locate the line that represents the liquid-gas equilibrium on the phase diagram: This line is often called the vaporization curve. It separates the liquid phase from the gas phase.
Find the point on the vaporization curve that corresponds to 1 atm of pressure: This is where the normal boiling point is located on the phase diagram.
Read the temperature value at this point: The temperature at which the vaporization curve intersects the 1 atm pressure line is the normal boiling point of neon.
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Related Practice
Textbook Question
Referring to Figure 11.29, describe the phase changes (and the temperatures at which they occur) when CO2 is heated from -80 to -20°C at (a) a constant pressure of 3 atm,
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Textbook Question
The phase diagram for neon is
Use the phase diagram to answer the following questions. (a) What is the approximate value of the normal melting point?
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Textbook Question
Use the phase diagram of neon to answer the following questions. (b) What can you say about the strength of the intermolecular forces in neon and argon based on the critical points of Ne and Ar (see Table 11.5.)?
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Textbook Question
At 25 °C gallium is a solid with a density of 5.91 g/cm3. Its melting point, 29.8 °C, is low enough that you can melt it by holding it in your hand. The density of liquid gallium just above the melting point is 6.1 g/cm3. Based on this information, what unusual feature would you expect to find in the phase diagram of gallium?
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Open Question
In terms of the arrangement and freedom of motion of the molecules, how are the nematic liquid crystalline phase and an ordinary liquid phase similar? How are they different?