Why does 1 mol of any gas occupy a volume of approximately 22.4 L under standard conditions?
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Why does 1 mol of any gas occupy a volume of approximately 22.4 L under standard conditions?
Through numerous experimental measurements, it was found that when the amount of gas is 1 mol, its volume is 22.4 L. Moreover, at the same temperature and pressure, gases with the same volume contain the same number of molecules; it is specified that under standard conditions, 1 mol of a gas contains 6.02*10^23 molecules of that gas.
Natural laws. Many natural laws can only be discovered, not explained.
This spirit of seeking knowledge is worth learning from*, but for now, it is already quite remarkable that humanity has been able to discover this principle
I studied it in more detail again. As for why, under standard conditions, 1 mole of any gas occupies a volume of about 22.4 L, the reason is that the distance between gas molecules is much larger than the size of the molecules themselves. Therefore, the molar volume of a gas is determined by the average distance between these molecules, and this average distance depends on the temperature and pressure of the gas, with no relation to other properties of the gas. Under standard conditions, the molar volume of a gas is approximately 2.4 L. I think this is a more scientific explanation, which I’d like to share with everyone.
This is merely the result of calculating using the ideal gas law; it does not take into account intermolecular interactions or the volume of the molecules themselves, and is only applicable to ideal gases