Question

Applications 5.91 Would behave more like an ideal gas at Skor SOK? Explain your reasoning. 592 Would co behave more like an ideal gas at 2 atm or 20 atm? Explain your reasoning. The Liquid State Foundations 5.93 Compare the strength of intermolecular forces in liquids with those in gases. Compare the strength of intermolecular forces in liquids with those in solids. What is the relationship between the temperature of a liquid and the vapor pressure of that liquid? 5.96 What is the relationship between the strength of the attractive forces in a liquid and its vapor pressure? 5.97 Describe the process occurring at the molecular level that accounts for the property of viscosity. 5.98 Describe the process occurring at the molecular level that accounts for the property of surface tension Applications Questions 5.99-5.102 are based on the following: H-CH H- C-a H -C-0-H methane chloromethane methanol 5.99 Which of these molecules exhibit London dispersion forces? Why? 5.100 Which of these molecules exhibit dipole-dipole forces? Why? 5.101 Which of these molecules exhibit hydrogen bonding? Why? 5.102 Which of these molecules would you expect to have the highest boiling point? Why? Questions 5.103 and 5.104 are based on the following: HHH HHH HC-CC-HH-C-CC-HH-C-C HHH propane Isopropyl alcohol

Answer 1

5.91 co would exhibit ideal behaviour at higher temperature conditions because at very low temperatures, it will have forces of attraction and tends to show real gas behavior . Though both temperatures are low, it will have a better tendency to exhibit sideal behaviour at 50k. (higher of the two conditions ginen) 5.93 Intermolecular forces are stronger in liquids than in gases due to which liquids have properties like surface tension, viscosity, higher density than gases 5.95 Vapour pressure depends on intermolecular forces, fligh the intermolecular forces, lower will be V.P., At higher temperatures, intermolecular forces decreases and that vip will increase (v. P il directly proportional to temperature) 5.99 London dispersion forces predominantly erants in methane because cta in a non-polar molecule with no dipole moment. A temporory dipole moment is deneloped when two CA14 molecules approach each other. These are very weak intermolecular forces

aline 5.101 Methanol will exhibit hydrogen bonding because hydrogen is bonded to electron oxygen there fore bond becomes highly polar and thus denelops high dipole moment leading to t-bonding.