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13. Liquids, Solids & Intermolecular Forces

Phase Diagrams

13. Liquids, Solids & Intermolecular Forces

Phase Diagrams

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States of Matter of Phase Diagrams

States of Matter of Phase Diagrams

Phase Diagrams Example 1

Phase Diagrams Example 1

Phase Diagrams Concept 2

Phase Diagrams Concept 2

Phase Diagrams Example 2

Phase Diagrams Example 2

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The Phase Diagram of Water

The Phase Diagram of Water

What are phase diagrams? - Real Chemistry

What are phase diagrams? - Real Chemistry

11.2 Phase Diagrams | General Chemistry

11.2 Phase Diagrams | General Chemistry

Phase diagrams | States of matter and intermolecular forces | Chemistry | Khan Academy

Phase diagrams | States of matter and intermolecular forces | Chemistry | Khan Academy

Phase Changes, Heats of Fusion and Vaporization, and Phase Diagrams

Phase Changes, Heats of Fusion and Vaporization, and Phase Diagrams

Professor Dave Explains

Phase Diagrams of Water & CO2 Explained - Chemistry - Melting, Boiling & Critical Point

Phase Diagrams of Water & CO2 Explained - Chemistry - Melting, Boiling & Critical Point

The Organic Chemistry Tutor

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Practice this topic

Multiple Choice

The critical point of this substance occurs at what temperature?

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Multiple Choice

Arrow I corresponds to:

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Multiple Choice

What is the normal freezing point of this unknown substance?

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Multiple Choice

At what temperature can we no longer tell the difference between the liquid and gas phases?

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Multiple Choice

Which processes occur at the triple point?

Multiple Choice

The ability for liquids to mix without separating into two phases is called _________.

Multiple Choice

For a given substance:

Multiple Choice

Consider adding enough heat to a solid sample of a substance below its melting point to change the sample to the gas above its boiling point. Which of the following would involve no change in temperature of the sample as the described transition occurs?

Multiple Choice

Calculate the amount of heat (in J) required to heat 2.00 grams of ice from −12.0℃ to 88.0℃.
The heat of fusion of water is 6.02 kJ/mol, the specific heat capacity of ice is 2.09 J/g ▪℃ and the specific heat capacity of water is 4.184 J/g ▪℃.

Multiple Choice

Consider the phase diagram below: What changes would the sample undergo as the sample moves from the temperature and pressure at point 'a' to the temperature and pressure at point 'b'?

Textbook Question

Using this graph of CS2 data,

determine (a) the approximate vapor pressure of CS2 at 30°C,

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Textbook Question

The phase diagram of a hypothetical substance is

(b) What is the physical state of the substance under the following conditions? (i) T = 150 K, P = 0.2 atm; (ii) T=100K,P=0.8atm; (iii) T = 300K,P = 1.0atm. [Section 11.6]

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Textbook Question

This portion of a phase diagram shows the vapor–pressure curves of a volatile solvent and of a solution of that solvent containing a nonvolatile solute. (b) What are the normal boiling points of the solvent and the solution? [Section 13.5]

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Textbook Question

At standard temperature and pressure, the molar volumes of Cl2 and NH3 gases are 22.06 and 22.40 L, respectively. (d) Are the molar volumes in the solid state as similar as they are in the gaseous state? Explain.

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Textbook Question

Benzoic acid, C6H5COOH, melts at 122 °C. The density in the liquid state at 130 °C is 1.08 g/cm3. The density of solid benzoic acid at 15 °C is 1.266 g/cm3. (b) If you converted a cubic centimeter of liquid benzoic acid into a solid, would the solid take up more, or less, volume than the original cubic centimeter of liquid?

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Textbook Question

A phase diagram for a substance that exhibits the liquid crystalline state is shown. (b) If the substance is at a temperature and pressure repre- sented by point 1 and the temperature is increased until the phase changes, what is the phase transition? Describe how the ordering of molecules changes, and propose a reason for the change.

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Textbook Question

The following compound undergoes a phase transition from the solid to the smectic liquid crystal phase at 121 °C. Upon further heating, the compound undergoes another transition to liquid phase at 131 °C.

(a) Which image represents the arrangement of molecules at 125 °C?

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Textbook Question

Assume that you have a sample of gas at 350 K in a sealed container, as represented in (a). Which of the drawings (b)–(d) represents the gas after the temperature is lowered from 350 K to 150 K? The boiling point of the gas is 90 K.

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Textbook Question

The following phase diagram shows part of the liquid–vapor phase-transition boundaries for two solutions of equal con- centration, one containing a nonvolatile solute and the other containing a volatile solute whose vapor pressure at a given temperature is approximately half that of the pure solvent.

(d) Based on your drawing, what is the approximate normal boiling point of the pure solvent?

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Textbook Question

Water at room temperature is placed in a flask connected by rubber tubing to a vacuum pump, and the pump is turned on. After several minutes, the volume of the water has decreased, and what remains has turned to ice. Explain

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Textbook Question

(a)Two pans of water are on different burners of a stove.One pan of water is boiling vigorously, while the other is boiling gently. What can be said about the temperature of the water in the two pans?

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Textbook Question

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 evapo- rating from your cup and cooling it. (c) High in the moun- tains, 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.

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Textbook Question

Using the vapor-pressure curves in Figure 11.25, (d) estimate the external pressure at which diethyl ether will boil at 40 °C.

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Textbook Question

Appendix B lists the vapor pressure of water at various external pressures. (c) A city at an altitude of 5000 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?

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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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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

Benzene has a melting point of 5.53 °C and a boiling point of 80.09 °C at atmospheric pressure. Its density is0.8787 g>cm3 when liquid and 0.899 g>cm3 when solid; it has Tc = 289.01 °C, Pc = 48.34 atm, Tt = 5.52 °C, and Pt = 0.0473 atm. Starting from a point at 200 K and 66.5 atm, trace the following path on a phase diagram. (1) First, increase T to 585 K while keeping P constant. (2) Next, decrease P to 38.5 atm while keeping T constant. (3) Then, decrease T to 278.66 K while keeping P constant. (4) Finally, decrease P to 0.0025 atm while keeping T constant. What is your starting phase, and what is your final phase?

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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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Textbook Question

Consider the phase diagram shown here. Identify the states present at points a through g.

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Textbook Question

The table below lists the density of O2 at various tempera-tures and at 1 atm. The normal melting point of O2 is 54 K.

(b) Over what temperature range is O2 a liquid?

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Textbook Question

Nitrogen has a normal boiling point of 77.3 K and a melting point (at 1 atm) of 63.1 K. Its critical temperature is 126.2 K and its critical pressure is 2.55 * 104 torr. It has a triple point at 63.1 K and 94.0 torr. Sketch the phase diagram for nitrogen. Does nitrogen have a stable liquid state at 1 atm?

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Textbook Question

Argon has a normal boiling point of 87.2 K and a melting point (at 1 atm) of 84.1 K. Its critical temperature is 150.8 K and its critical pressure is 48.3 atm. It has a triple point at 83.7 K and 0.68 atm. Sketch the phase diagram for argon. Which has the greater density, solid argon or liquid argon?

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Textbook Question

Substance X has a vapor pressure of 100 mm Hg at its triple point (48 °C). When 1 mol of X is heated at 1 atm pres- sure with a constant rate of heat input, the following heating curve is obtained: (b) For each of the following, choose which phase of X (solid, liquid, or gas) fits the description. (iii) Has the greatest specific heat

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Textbook Question

The phase diagram for sulfur is shown here. The rhombic and monoclinic states are two solid states with different structures. a. Below what pressure does solid sulfur sublime?

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Textbook Question

The phase diagram for sulfur is shown here. The rhombic and monoclinic states are two solid states with different structures. b. Which of the two solid states of sulfur is more dense?

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Textbook Question

Naphthalene (C10H8) is the main ingredient in traditional mothballs. Its normal melting point is 81 °C, its normal boiling point is 218 °C, and its triple point is 80 °C at 1000 Pa. Using the data, construct a phase diagram for naphthalene, labeling all the regions of your diagram.

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Textbook Question

A particular liquid crystalline substance has the phase diagram shown in the figure. By analogy with the phase diagram for a nonliquid crystalline substance, identify the phase present in each area.

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Textbook Question

Liquid butane (C4H10) is stored in cylinders to be used as a fuel. The normal boiling point of butane is listed as -0.5 °C. (b) Suppose the valve to the tank is opened and a few liters of butane are allowed to escape rapidly. What do you expect would happen to the temperature of the remaining liquid butane in the tank? Explain.

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Textbook Question

Based on the phase diagram of CO2 shown in Figure 11.39(b), describe the state changes that occur when the temperature of CO2 is increased from 190 K to 350 K at a constant pressure of (a) 1 atm

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Textbook Question

Draw a phase diagram showing how the phase boundaries differ for a pure solvent compared with a solution.

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Based on the phase diagram shown below, how will the melting point of the substance change if the pressure is increased above 1 atm?

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In the phase diagram for water, indicate the direction that the solid–liquid and liquid–gas coexistence lines will move along the temperature axis after the addition of solute.

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A gaseous substance turns directly into a solid. Which term describes this change?

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The boiling temperature and its relationship to the system exist in the ____.

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Which term describes the process by which water vapor changes to the liquid state?

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Starting from the lower triple point, what action(s) would produce liquid carbon?

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Starting from the lower triple point, what action(s) would produce liquid carbon?

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What does water undergo when it turns to gas from liquid on surface of a sidewalk?

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What is it called when water vapor up in the sky becomes liquid water?

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Changes of phase most always require _________.

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