The Ideal gasThe ideal gas is derived from the kinetic theory of gases, that assumes:
The ideal gas is a hypothetical gas that consists of particles with mass without volume and attractive forces in between.
The "ideal gas" does not exist, because the ideal gas is based on assumptions that are not neccessarily true. Despite this, scientists can still make accurate predictions using this model, under normal circumstances and conditions. The ideal gas assumes that gas molecules do not attract or repel each other. This attraction/repulsion may be neglected when there is a large distance between gas molecules, but they become greater as the distance between molecules decrease. This is why there are often deviations from the ideal gas under certain extreme conditions. |
Critical temperatures high densities |
Low/High pressures |
The higher the pressure of a system is, the more the molecules are forced into contact, so the more they interact. Therefore, the ideal gas law becomes less accurate as pressure increases - high pressure causes gases to behave non-ideally.
At lower temperatures, the molecules of a gas are moving too slowly, making the intermolecular force of attraction much stronger. The molecules can no longer break their attractive interactions. At higher densities, the volume of gas is significant, making the gas behave non-ideally. |
Dalton's Law of Partial Pressures
Dalton's Law of Partial Pressures was discovered by John Dalton, and it states that the total pressure of a mixture of gases is equal to the sum of the individual pressures of each gas.
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Gas Stoichiometry: steps |
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