There are several gas laws including Boyle’e law, Charles’s Law, Avogadro’s Law, Lussac’s law and the ideal gas law. All the gasses in someway obey these laws. In order to understand how and why gases behave and are influenced by we must understand the gas laws.
In 1811 Avogadro’s research led to the discovery of his law which states that the number of moles are proportional to the volume of a gas at a constant temperature and pressure. V = kn where k is the constant of proportionality. Avogadro introduces the idea of particles and how they combine and react in a chemical reaction. A soft drink is an example of Avogadro’s law. When the soft drink is shaken molecules will be released into the air. Therefore the pressure in the bottle is proportional to the number of moles of molecules in the bottle.
Boyle’s Law published in
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Simply put, when a gas is heated, its particles gain more energy and the volume is forced to increase. A new temperature scale is introduced for these laws. The absolute temperature scale (T) (Kelvin temperature scale). T(K) = temperatureºC + 273.15. Kelvin allows all temperatures to be positive as 0K is the lowest temperature possible. This means that constant pressure, the volume of a fixed gas is proportionate to it’d absolute temperature. This creates the formula V2/T2 = V1/T1. A hot air balloon is a great example of Charle’s law seeing as after Charles saw a hot air balloon launch he was jealous and wanted to try and make one himself. This founded his launch of the first human carrying hydrogen balloon. When the hot flame is on the air inside the balloon the particles heat up and start moving faster taking up more space. This causes the balloon to inflate and the air inside the balloon to become less dense then the air around it. The hot air balloon then can rise due to the low density inside the