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Test Review Chapter 17
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Melting and Freezing Which is defined as the temperature at which the particles move fast enough to slip past each other?
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Vapor Equilibrium Define temperature.
Explain the dynamic equilibrium in a closed beaker containing water.
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Vapor Equilibrium H2O(l) H2O(g)
Show an equation for the reversible change of water in the liquid state to water in the vapor state. H2O(l) H2O(g)
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Equilibrium Define Le Chatelier’s principle.
Explain how ice skating works according to Le Chatelier’s principle.
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Changing State Why do substances with strong intermolecular forces have low vapor pressures? Define melting point.
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Changing State Name the phase change in: Boiling Melting Subliming
Depositing
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Changing State Name the phase change in: Freezing Condensing
Evaporating Liquefaction
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Changing State Define Boiling point. Define normal boiling point.
Define volatile.
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Liquefaction What is the critical point?
Why would you want to liquefy a gas?
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Boiling At what temperature does water boil? What is a phase diagram?
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Vapor Pressure Chart When the pressure is 90 kPa, what is the boiling point of CCl4? What is the normal boiling point of each gas?
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Heat Calculations How much heat, in KJ, is needed to melt 5.67 grams of FeO? ΔHfus = 32.2 KJ/g Watch the units of the constant………
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Heat Calculations How much heat, in KJ, is needed to change the temperature of 55.5 grams of water from 20OC to 99OC ? The C of water = 4.18 J/gOC
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Heat Calculations How much heat, in KJ, is needed to boil 58.5 grams of water? ΔHvap= 2260 J/g
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Heat Calculations A piece of unknown metal with a mass of 23.8 grams is heated to 100oC and dropped into 50.0 grams of water at 24.0oC. The final temp is 32.5oC. Find the C of the metal. C of water = 4.18 J/goC
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Heat Calculations A piece of copper with a mass of 50.0 grams is heated to 450oC and dropped into grams of water at 24.0oC. Find the final temperature. C of water = 4.18 J/goC C of copper = J/goC
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Intermolecular Forces
List the following from weakest to strongest: Hydrogen bonds Covalent bonds van der Waals forces Dipole-dipole forces London forces
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Intermolecular Forces
Define: London forces
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Intermolecular Forces
Define: Dipole-dipole forces
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Intermolecular Forces
Define: Hydrogen bonding
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Intermolecular Forces
Explain the trend in this graph:
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Intermolecular Forces
What properties of water can be attributed to hydrogen bonding?
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