Unit 4- Gasses and Kinetic Molecular Theory Exam Update

Unit 4- Gasses and Kinetic Molecular Theory Exam Update
Properties of gases - Correct Answer-indefinite volume: gases volume is indefinite since
it can be changed fairly easily
Pressure - Correct Answer-changing the pressure can affect the volume
increase pressure->volume decreases
decrease pressure->volume increases
the space between particles is very large which allows the pressure to change
Volume of gases is affected by - Correct Answer-pressure and the amount of gas( the
number of particles, the more particles the more volume)(when both pressure and temp
are constant)
Temperature: measurement of the average kinetic energy
high temp->fast particles, increase volume
low temp->slow particles, decrease volume
volume of container - Correct Answer-gas takes the volume of its container which limits
the volume of a gas (rigid container)
Kinetic Molecular Theory - Correct Answer-a theory used to help explain how ideal
gases behave
requirements of KMT(for ideal gases) - Correct Answer-1) particles move in random
straight lines of motion
2) gas particles are separated by a great distance, relative to their size
3) The gas particles are not attracted to each other
4) Collisions transfer energy from high velocity particles to low velocity particles
Pressure - Correct Answer-pressure defined by KMT is cause by the random collision of
particles with the containers wall
more collisions higher pressure, less collision less pressure
gases that behave like an ideal gas - Correct Answer-H2(hydrogen)
He(helium)
most gases violate KMT because particles do have attraction towards each other
Condition for gasses to behave like an ideal gas - Correct Answer-high temp low
pressure
Boyle's law - Correct Answer-states that for a given mass at a constant temp the volume
of a gas is inversely related to pressure
p1(v1)=p2(v2)
Charles Law - Correct Answer-
Charles Law - Correct Answer-states that a gases volume and temperature have a
direct relationship
as temp increases volume increases proportionally

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