Chemistry
Practice Sheet for Test Chapter 10
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Practice sheet before Test Chapter 10 Kinetic Theory
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previous homework to help you study for the test
Write all answers on lined paper:
1) Conversions: K= °C + 273
e)
f)
g)
h)
i)
°C = K - 273
Convert to Kelvin temperature:
a) 570 °C
Convert to Celsius temperature:
c) 145 K (Kelvin)
Which temperature scale has no negative numbers?
What is the lowest possible Kelvin temperature?
What is the lowest Celsius temperature?
What is the SI unit for temperature?
What is the metric unit (but not SI) for temperature?
b) -15 °C
d) 350 K
include unit K
include unit°C
2) Word bank: kinetic theory, absolute zero, intermolecular forces, vapor pressure, vacuum, atmospheric
pressure, kinetic energy, gas pressure. condensation, boiling point, normal boiling point, sublimation
a)
b)
c)
d)
e)
f)
g)
h)
i)
k)
l)
m)
The pressure above a liquid in a sealed container
The attractive forces between molecules
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The change of a gas or vapor to the liquid state
boiling point of a liquid at standard atmospheric pressure of 101.3 kPa
A space where no particles of matter exist
The energy an object has because of its motion
The force resulting from collisions of gas particles per surface unit of a container wall
The pressure that results from the collisions of air molecules with objects
Theory that particles of all forms of matter are in constant motion
The temperature at which all motion of particles should stop
The change of matter from a solid directly to a gas without becoming a liquid
3) a) Explain the three points of the kinetic model of Ideal Gases: 1.
…,2.…,
3.
…
b) Use the kinetic theory to explain why you can smell an open perfume bottle across the room
c) How do ideal gases differ from real gases?
4) Word bank: gas, liquid, solid, diffusion, amorphous, liquid crystals, volatile, plasma, sublimation
a) Rigid with a definite shape and volume, and its particles are fixed in place.
b) Flowing matter with a definite volume but an indefinite shape, and it takes the shape of the container.
c) Flowing, compressible matter with neither definite volume or shape, which takes the volume of the container
d) Ionized gas, but electrically neutral because it contains equal amount of free electrons and positive ions,
forms at very high temperatures. Most common form of matter in the Universe but least common on Earth
e) Structure in only one or two dimensions, arranged either in layers or parallel lines (used in LCD)
f) Solids with disjointed and incomplete crystal lattice (e.g. wax, rubber, plastic, asphalt, glass)
g) Conversion from a solid to a gas without being liquid in-between.
h) Process by which particles of matter fill a space because of random motion
i) A liquid that evaporates quickly
Chemistry
Practice Sheet for Test Chapter 10
5) Describe the movement of particles in a) a gas b) a liquid
Jaeger
c) a solid.
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7) Define each and differentiate between a) Vaporization, b) Evaporation, and c) Boiling.
8) How does the atmospheric pressure change as you climb up a mountain? (increases/decreases)
9) a) When the temperature in a closed container increases, its average kinetic energy___. (increases/decreases)
b) When the temperature in a closed container increases, its vapor pressure ___. (increases/decreases)
c) Kelvin temperature directly relates to average kinetic energy.
Therefore, when the Kelvin temperature doubles, the average kinetic energy ____ (will be half/ doubles).
d) When the Kelvin temperature decreases by half, the average kinetic energy ____ (will be half/ doubles).
10) a) How can you lower the boiling point of a liquid?
b) How can you raise the boiling point of a liquid?
11) True or False? The kinetic energy depends on speed and mass. Therefore, at the same average kinetic
energy (same temperature), smaller particles (hydrogen) will on an average move at a higher speed than
particles with a higher mass (oxygen).
12) endothermic or exothermic?
a) melting
e) sublimation
b) evaporating
c) boiling
f) condensation
g) freezing
Energy
d) vaporization
13) Heat of fusion or heat of vaporization
a) Same amount of energy is needed to break apart the crystal lattice.
b) Needed to overcome the intermolecular forces in liquids and the outside pressure
c) The energy released when 1 kg of a liquid solidifies at its normal freezing point.
d) Energy absorbed when 1 kg of a liquid vaporizes at its normal boiling point
14) a) Is evaporation an endothermic or exothermic process? b) Explain why.
c) Give one example where the cooling effect during evaporation is useful.
15) Describe and interpret the following diagrams
a) Heating Curve of Water
b) Kinetic Energy and Evaporation