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Unit 4 assignment
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Overall expectation 1:1) Compare a solid and a gas with respect to the arrangement of their molecules. Use
this comparison to explain how solids exert pressure and how gasses exert pressure.
Solids Gasses
Molecules of solids are tightly packed Molecules of gasses are free.
together.
Energy in solids travel very fast because of Energy in gasses travel very slow because the
the particles being packed together. particles are free and take time to interact with
other particles.
The molecules of solids are neatly organized Molecules of gasses are not organized and
because the molecules of solids are held can’t be set together because the molecules
tightly together. are free.
Describe condensation (the change from gas to liquid) in terms of the kinetic molecular theory (KMT). Heat is
needed to excite particles of gasses and set them free so as heat is removed from the gas, the molecules of gas
start to move more slowly causing the intermolecular forces to be strong enough to pull the molecules together
to form droplets of liquid which eventually collect and form a lot of liquid. Explain, using the KMT, why a gas
is compressible and a liquid is not. According to the KMT the molecules of gas are free and far apart from each
other so when we try to compress the molecules they will be forced to be close to each other. According to the
KMT, the molecules of liquid are already close to each other so when we try to compress more it will not be
possible.
2) Driving a car causes the tires to get hot from friction. If you want to check to see if your tires
need air, the service manual of your car warns you against checking the tire pressure when the
tire is hot. Explain why, using your understanding of KMT. Heat is needed to excite the
molecules of gas and spread in the tire, this causes a lot of pressure to build up in the tire and
when we try to check the tire when it is hot there will be a higher inaccurate reading.
3) Explain how and why the number of moles of gas affects the volume of that gas, assuming
that the container volume can change. Is the relationship between number of moles and volume
direct or indirect? The number of moles affect the volume of the gas because as mentioned in
Avogadro’s law “the volume of a gas changes if the number of moles of the gas change when the
pressure and the temperature are about the same. The relationship is direct.
4) Explain how the molar volume of a gas would change as the temperature increases. As the
temperature of the gas increases, the molecules of the gas have more energy and start to move
faster. As a result, the molecules strike the surface of the container with more force. If the
container expands, the volume increases.
Overall expectation 2:
1) A steel container of compressed gas with an initial pressure of 369 kPa is heated from
15.0°C to 42.5°C because of storage in a sunny area. Calculate the new pressure in the container.
Remember that temperature needs to be in Kelvin when working with the gas laws!
P₁ = 369 kPa, T₁ = 15.0℃ = 15.0 + 273 = 288 K, P₂ = ?, T₂ = 42.5℃ = 42.5 + 273 = 315.5 K
𝑃1𝑇2 (369 𝑘𝑃𝑎)(315.5 𝐾)
P₂ = 𝑇1
= (288𝐾)
= 404 kPa
2
Therefore, the new pressure of the gas is 4.04✕10 kPa.
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