Question

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Applications 5.91 Would behave more like an ideal gas at 5 Kor 50 K? Explain your reasoning 5.92 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 5.94 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? 3.97 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 - C- H H- C- a H C - O-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 Hн Н -CC- CH=CC=CH- pe Isopropulalah propylene glycol

Answer 1

At low temperature there is significant deviation shown by real gas from ideal behavior. It
Is due to the role of intermolecular forces which becomce more imporant at
low temperature. Ideal behavior is explained under the assumption that;there
is no forces of attraction between gas particles
At higher temperature intermolecular forces are less important.Hence gas behave
ideally at higher temperature. So Co behave ideally at 50 K than 5 K
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5.93)
Strength of intermolecular forces in gases are weaker than the intermolecular
forces present in liquld states. It is because, in liquid , the particles
are more closer than the gaseous particles. Thus force between these
particles are higher in liquids.

5.95)
vapor pressure is the pressure exerted by the vapor formed above the liquid
More the vapor ,more the pressure.When temperature of liquid increases , more
vapor will be formed .SO vapor pressure increases when temperature increases
5.97)
Viscosity is a property shown by liquids .It depends on intermolecular forces
between the liquid particles> Stronger the inter molecular force, more viscus
the liquid will be.SO if the liquid with H.bonding will have more viscosity than
the liquid which does not show H.bonding
5.99)
CH4. shows london forces.It is the weakest intermolecular force. Ch4 molecule
is a non polar molecule so there is no dipole-dipole force . Also in CH4 there
is no electro negative atom like N,F or O to show hydrogen bonding

5.101)

Methanol has H attached to a more electro negative atom Oxygen .SO there is
hydrogen bonding in methanol

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