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Gas Laws
Gas laws are a set of equations describing the relationships among the pressure, volume, and
temperature of a gas
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The kinetic theory of gases stipulates that a gas is made up of very small particles in constant, rapid
random motion
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Boyle’s Law
Boyle's law, also referred to as the Boyle–Mariotte law, or Mariotte's law (especially in France), is an
experimental gas law that describes how the pressure of a gas tends to decrease as the volume of the
container increases
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The equation asserts that for a given mass of confined gas, the product of pressure and volume is a
constant, and this stays true as long as the temperature remains constant
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Similarly, when the volume of the gas diminishes, the pressure of the gas rises
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Real-Life Application
When you fill your bike tires with air, you may see a real-world implementation of Boyle's Law
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This raises the pressure of the gas, causing it to push against the tire's walls
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A Coke bottle is another example
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It is extremely difficult to squeeze the bottle when it is closed because the
gas is confined to limited space and pushes against the bottle's walls
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Its pressure is decreasing at the same time
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When the pressure on a sample of a dry gas is maintained constant, the temperature and
volume will be in direct proportion, according to a modern formulation of Charles' law
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The law can be expressed as follows for comparing the same material under
two distinct sets of conditions:
V=kT
where:
● V is the volume of the gas,
● T is the temperature of the gas (measured in kelvins), and
● k is a non-zero constant
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Real-Life Application
A bread product is one of the delectable Charles law instances in real life
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The applicability of Charles Law in real life may also be seen in our kitchen
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Carbon dioxide gas is produced by yeast
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As a result of this enlargement, our bread and
cakes seem pleasantly spongy and fluffy and are ready to serve
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It may
be stated mathematically as P/T = k
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Gay-Lussac is wrongly credited with the formulation of the Pressure Law, which showed that the
pressure of an enclosed gas is exactly related to its temperature and which he was the first to propose
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Gay-Lussac's Law is a gas law named after French chemist Joseph Louis Gay-Lussac
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Tire pressure in automobiles falls on cold days and rises on hot days
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Similarly, if your
tires are properly filled when hot, they will be underinflated when cold
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When a pressure cooker is heated, the pressure inside the device rises
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Because the container
is sealed, steam does not lose flavors to the air
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A pressure cooker is similar to an electric water heater
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If the valve fails, heat causes the steam pressure inside the heater to rise,
finally bursting it
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The
law is an example of the ideal gas law
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" For a given mass of an ideal gas, the volume and quantity
(moles) of the gas are exactly proportional if temperature and pressure remain constant
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Equal
quantities of gaseous hydrogen and nitrogen, for example, have the same number of atoms when they
are at the same temperature and pressure and exhibit perfect gas behavior
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Real-Life Application
Blowing up a balloon is the greatest example of Avogadro's law
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Similarly, as you deflate a balloon, gas escapes and the volume diminishes
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Although it has significant drawbacks, it is a decent approximation of the behavior of various
gases in many situations
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The ideal gas law is frequently
expressed empirically:
PV = nRT
where P, V, and T denote pressure, volume, and temperature, respectively; n denotes the amount of
substance; and R is the ideal gas constant
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It may also be deduced from
microscopic kinetic theory, as August Krönig and Rudolf Clausius did (seemingly independently) in
1856 and 1857, respectively
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In real life, the ideal gas law has various uses
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Ideal gas laws are applied in the operation of airbags in automobiles
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As the airbags
expand, they fill with nitrogen gases
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While the sodium metal reacts with potassium nitrate
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Buildings and Planes
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Ventilation units must be
placed in commercial buildings if air ventilation is insufficient to keep the amount of oxygen and
carbon dioxide in the building balanced
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