# D starting at d if the pressure is lowered while the

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Chapter 4 / Exercise 7
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d. Starting at D, if the pressure is lowered while the temperature remains constant, describe what will happen.Ans:
Difficulty: E78.Draw a fully labeled phase diagram (Pversus T) of a substance whose solid phase can melt due to applied pressure (i.e., solid is less dense than liquid). Clearly label the triple point and the critical temperature on your diagram.Ans:Difficulty: E79.Liquid ammonia boils at –33.4°C and has a heat of vaporization of 23.5 kJ/mol. Calculate its vapor pressure at –50.0°C.Ans:316 torrDifficulty: MPage 181
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Chapter 4 / Exercise 7
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Chapter 12: Intermolecular Forces: Liquids, Solids, and Phase Changes80.Chlorine trifluoride is used in processing nuclear reactor fuel. It has a vapor pressure of 29.1 torr at –47.0°C and its heat of vaporization is 30.61 kJ/mol. At what temperature would its vapor pressure be 107.7 torr?
Difficulty: M81.The vapor pressure of 1-butene is 1.268 atm at 273.15 K and its heat of vaporization is 22.9 kJ/mol. What is the normal boiling point of 1-butene?
Difficulty: M82.a. State the essential requirements for hydrogen bonding to be important in a compound.b. List four properties of water which are significantly influenced by the presence of hydrogen bonding.
Difficulty: E83.a. Explain what is meant by the term “unit cell”.b. Copper metal has a face-centered cubic unit cell. The edge length of the unit cell is 361 pm, and the atomic weight of copper is 63.55 amu. Calculate the density of the copper in g/cm3.
c. From the data in (b), calculate the radius of a copper atom in pm.Ans:
b. 8.97 g/cm3c. 128 pmDifficulty: H84.Strontium metal crystallizes in a cubic unit cell which has an edge length of 612 pm. If the mass of an atom of Sr is 87.62 amu, and the density of Sr metal is 2.54 g/cm3, calculate the number of atoms per unit cell. (1 amu = 1.661 10–24g.)Ans: 4Difficulty: HPage 182
Chapter 12: Intermolecular Forces: Liquids, Solids, and Phase Changes85.Iron has a body-centered cubic unit cell, and a density of 7.87 g/cm3. Calculate the edge length of the unit cell, in pm. (The atomic mass of iron is 55.85 amu. Also, 1 amu = 1.661 10–24g.)Ans:287 pmDifficulty: H
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