Question 1

Explain why the boiling point of nitrogen (N₂, 77 K) is much lower than that of carbon monoxide (CO, 84 K) even though both have the same number of electrons and protons and nearly the same mass.

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Question 2

For each of the following pairs of compounds, identify the one that is more likely to be soluble in water. Explain the rationale for your choice. A) CCl₄ or CHCl₃ B) CH₃OH or C₅H₁₁OH C) NaF or MgO

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Question 3

Would water rise to the same height in a capillary tube made of polyethylene plastic as it does in a glass capillary tube of the same diameter? Polyethylene is a hydrocarbon, and glass is mostly silicon dioxide. Explain.

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Question 4

Water at 20°C exposed to air at 1.0 atm pressure can contain a maximum of 8.6 mg/L of oxygen. Calculate the value of Henry's law constant (mol/L · atm) for oxygen at this temperature. The mole fraction of oxygen in air is 0.209.

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Question 5

Describe the similarity and the difference between sublimation and evaporation.

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Question 6

What structural characteristics must a molecule have in order to hydrogen bond?

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Question 7

Henry's law constant for oxygen dissolving in blood is 0.0374 mol/(L · atm) at body temperature (37°C). Calculate the molar concentration of oxygen in the blood of a scuba diver. Air pressure is 2.5 atm for the scuba diver. The mole fraction of oxygen in air is 0.209.

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Question 8

Why do gases behave nonideally at high pressures and low temperatures?

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Question 9

Arrange the first four halogens in order of increasing boiling point.

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Question 10

Arrange the following compounds in order of increasing attraction between their ions: MgO, CaO, BaO.

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Question 11

Which liquid, water or ethanol, would you expect to have the higher surface tension and viscosity? Explain.

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Question 12

CH₂F₂ has a dipole moment of 1.93 D and a boiling point of -52°C. CH₂Cl₂ has a dipole moment of 1.60 D and a boiling point of 40°C. Why is the boiling point of dichloromethane so much higher than that of difluoromethane?

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Question 13

Henry's law constant for oxygen dissolving in blood is 0.0374 mol/(L · atm) at body temperature (37°C). Calculate the ratio of the molar concentration of oxygen in the blood of a mountain climber to that of a scuba diver. Air pressure on the mountain is 0.35 atm and is 3.0 atm for the scuba diver. The mole fraction of oxygen in air is 0.209.

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Question 14

Why does HI boil at a higher temperature than HBr, yet the dipole moment of Hbr (0.82 D) is larger than that of HI (0.38 D)?

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Question 15

Henry's law constant for oxygen dissolving in blood is 0.0374 mol/(L · atm) at body temperature (37°C). Calculate the molar concentration of oxygen in the blood of a mountain climber. Air pressure on the mountain is 0.40 atm. The mole fraction of oxygen in air is 0.209.

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Question 16

Identify the dominant intermolecular interaction or interactions that must be overcome when solid CO₂ sublimes and H₂O melts.

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Question 17

For each of the following pairs of compounds, identify the one that is more likely to be soluble in water. Explain the rationale for your choice. A) Br₂ or NaBr B) CH₃CH₂OH or CH₃OCH₃ C) CO₂ or KOH

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Question 18

Sketch a phase diagram for water and correctly label all the parts (areas, lines, points, key temperatures).

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Question 19

Why do the strengths of dispersion interactions generally increase with the molar mass of the compound?

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Question 20

Henry's law constant for oxygen dissolving in water is 1.3 * 10^-³ mol/L · atm at 20°C. What is the maximum molar concentration of oxygen in a pond at this temperature? The mole fraction of oxygen in air is 0.209.

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Quiz 10: Forces Between Ions and Molecules

Explain why the boiling point of nitrogen (N2, 77 K) is much lower than that of carbon monoxide (CO, 84 K) even though both have the same number of electrons and protons and nearly the same mass.

For each of the following pairs of compounds, identify the one that is more likely to be soluble in water. Explain the rationale for your choice. A) CCl4 or CHCl3 B) CH3OH or C5H11OH C) NaF or MgO

Would water rise to the same height in a capillary tube made of polyethylene plastic as it does in a glass capillary tube of the same diameter? Polyethylene is a hydrocarbon, and glass is mostly silicon dioxide. Explain.

Water at 20°C exposed to air at 1.0 atm pressure can contain a maximum of 8.6 mg/L of oxygen. Calculate the value of Henry's law constant (mol/L · atm) for oxygen at this temperature. The mole fraction of oxygen in air is 0.209.

Describe the similarity and the difference between sublimation and evaporation.

What structural characteristics must a molecule have in order to hydrogen bond?

Henry's law constant for oxygen dissolving in blood is 0.0374 mol/(L · atm) at body temperature (37°C). Calculate the molar concentration of oxygen in the blood of a scuba diver. Air pressure is 2.5 atm for the scuba diver. The mole fraction of oxygen in air is 0.209.

Why do gases behave nonideally at high pressures and low temperatures?

Arrange the first four halogens in order of increasing boiling point.

Arrange the following compounds in order of increasing attraction between their ions: MgO, CaO, BaO.

Which liquid, water or ethanol, would you expect to have the higher surface tension and viscosity? Explain.

CH2F2 has a dipole moment of 1.93 D and a boiling point of -52°C. CH2Cl2 has a dipole moment of 1.60 D and a boiling point of 40°C. Why is the boiling point of dichloromethane so much higher than that of difluoromethane?

Why does HI boil at a higher temperature than HBr, yet the dipole moment of Hbr (0.82 D) is larger than that of HI (0.38 D)?

Henry's law constant for oxygen dissolving in blood is 0.0374 mol/(L · atm) at body temperature (37°C). Calculate the molar concentration of oxygen in the blood of a mountain climber. Air pressure on the mountain is 0.40 atm. The mole fraction of oxygen in air is 0.209.

Identify the dominant intermolecular interaction or interactions that must be overcome when solid CO2 sublimes and H2O melts.

For each of the following pairs of compounds, identify the one that is more likely to be soluble in water. Explain the rationale for your choice. A) Br2 or NaBr B) CH3CH2OH or CH3OCH3 C) CO2 or KOH

Sketch a phase diagram for water and correctly label all the parts (areas, lines, points, key temperatures).

Why do the strengths of dispersion interactions generally increase with the molar mass of the compound?

Henry's law constant for oxygen dissolving in water is 1.3 * 10-3 mol/L · atm at 20°C. What is the maximum molar concentration of oxygen in a pond at this temperature? The mole fraction of oxygen in air is 0.209.

Explain why the boiling point of nitrogen (N₂, 77 K) is much lower than that of carbon monoxide (CO, 84 K) even though both have the same number of electrons and protons and nearly the same mass.

For each of the following pairs of compounds, identify the one that is more likely to be soluble in water. Explain the rationale for your choice. A) CCl₄ or CHCl₃ B) CH₃OH or C₅H₁₁OH C) NaF or MgO

CH₂F₂ has a dipole moment of 1.93 D and a boiling point of -52°C. CH₂Cl₂ has a dipole moment of 1.60 D and a boiling point of 40°C. Why is the boiling point of dichloromethane so much higher than that of difluoromethane?

Identify the dominant intermolecular interaction or interactions that must be overcome when solid CO₂ sublimes and H₂O melts.

For each of the following pairs of compounds, identify the one that is more likely to be soluble in water. Explain the rationale for your choice. A) Br₂ or NaBr B) CH₃CH₂OH or CH₃OCH₃ C) CO₂ or KOH

Henry's law constant for oxygen dissolving in water is 1.3 * 10^-³ mol/L · atm at 20°C. What is the maximum molar concentration of oxygen in a pond at this temperature? The mole fraction of oxygen in air is 0.209.