Using real world examples, describe how changes in temperature, volume and pressures effect the behavior of a gas according to the following laws: Boyle's Law, Charles' Law, and Gay-Lussac's Law.

There are three laws that explain the behaviour of ideal gases:

1) Boyle's law:

"For a constant mass of ideal gas kept at constant temperature, the pressure of the gas is inversely proportional to the gas volume"

Mathematically:

where

p is the pressure of the gas

V is its volume

An example of application of Boyle's law is in the gas inside a syringe: if we block the nozzle of the syringe, and we push on the other side, we compress the volume of the gas inside; as a result, we notice that it becomes more and more difficult to push the other side of the syringe: this is because the pressure of the gas inside is increasing, due to Boyle's law.

2) Charle's Law:

"For a constant mass of an ideal gas kept at constant pressure, the volume of the gas is proportional to its absolute temperature"

Mathematically:

where

V is the volume of the gas

T is its absolute temperature (in Kelvin)

An easy example of application of Charle's law is a helium balloon. If we fill a balloon with helium gas, then we bring the ballon to another place with lower temperature, we notice that the balloon shrinks: this is because the temperature of the gas has decreased, and therefore the volume of the balloon decreases as well. Vice-versa, if we bring the balloon to a warmer place, it expands: the temperature has increased, and therefore the volume increases as well.

3) Gay-Lussac's law:

"For a constant mass of an ideal gas kept at constant volume, the pressure of the gas is proportional to its absolute temperature"

Mathematically:

where

p is the pressure of the gas

T is the absolute temperature of the gas (in Kelvin)

An example of Gay-Lussac's law in daily life is a canister containing gas. The canister has a fixed volume, so does the gas inside. If the canister is placed above a flame, heat is transferred to the gas inside the canister: as  result, the temperature of the gas increases. According to Gay-Lussac's law, the pressure increases as well: therefore, at some point, the pressure of the gas will be large enough to break the canister, which will then explode.

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