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Air is a mixture of non-reacting gases. Nitrogen, Oxygen, Carbon dioxide, Argon, water vapors and pollutants to name a few. The total pressure exerted by the air is the total sum of pressure of each individual gas. If there was no such thing as air pressure, you would choke because there's no air to breathe. At the same time, your body would expand because of the internal air pressure of 14.7 pounds per square inch inside that is not balanced by any air pressure at all outside.

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This law states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the all partial pressures of the individual gases present.

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If an engineer has to store 600g of oxygen in a container and that oxygen needs to be kept at a pressure of 1 atm and a temperature of 125 degrees Fahrenheit, the Ideal Gas Law is used to figure out what volume of a container needs to be built without collapsing or generating an issue.

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Useful for pure gas under one set of conditions. According to this law, when a gas is compressed into a smaller volume, the number and velocity of molecular collisions increase, raising the gas's temperature and pressure.

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At the bottling company, high-pressure carbon dioxide is added to the head space in order to ensure that more CO2 will be absorbed into the soda itself.
Once the container is opened, the pressure in the head space drops dramatically. Over a period of time, the soda will release the gas and will eventually go "flat".

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It comes from putting together three different laws about the pressure, volume, and temperature of the gas. They explain what happens to two of the values of that gas while the third stays the same. The three laws are:

Charles's Gas Law

Boyle's Gas Law

Gay-Lussac's

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As you blow up a basket ball you are forcing more air molecules inside the basketball. The more molecules the greater the volume, therefore the basketball expands.

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Pressure cookers are normally sealed so that the volume inside remains constant. Pressure inside the cooker will increase as the temperature increases, thus cooking the food inside quicker.

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A hot air balloon demonstrates that if we heat a gas, the volume of the balloon will expand.

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As the volume of the air trapped inside the bicycle pump is reduced, its pressure goes up and air is forced inside the tire.

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The pressure of a fixed amount of gas at a constant volume is directly proportional to its absolute temperature.
As temperature increases, then pressure increases while the number of gas molecules and volume remain constant.

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The volume is directly proportional to the number of gas molecules.
Equal volumes of gas contain equal number of gas molecules as pressure and temperature remain constant.

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The volume of a gas is directly proportional to its temperature.
As temperature increases, volume also increases while the pressure and number of moles remain constant.

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The pressure of a gas is inversely proportional to its volume.
As pressure increases,
volume decreases by the same factor while the temperature and number of moles remain constant.