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## Why does one mole of any gas always occupy the same volume 22.4 L at standard temperature and pressure?

According to my thinking, it may be **due to equal diffusion of all particles when at a particular temperature and pressure**. So going by this, one mole of all gases should occupy the same x L at some other temperature-pressure conditions.

## Why are moles 22.4 liters?

Always the Standard temperature and pressure (STP) is defined as 0°C (273.15 K) and 1 atm pressure. The molar volume of a gas is the volume of one mole of a gas at STP. At STP, one mole (6.02 × 10^{23} representative particles) of any gas occupies a volume of 22.4 L.

## Why does 1 mole of any gas occupy the same volume?

So the volumes have equal moles of separate particles (molecules or individual atoms) in them. Therefore one mole of any gas (formula mass in g), at **the same temperature and pressure** occupies the same volume .

## Why does 1 mole of any gas at STP fill up 22.4 L of volume?

The molar volume of a gas is the volume of one mole of a gas at STP. … Avogadro’s hypothesis states that equal volumes of **any gas at the same temperature and pressure contain the same number of particles**. At standard temperature and pressure, 1 mole of any gas occupies 22.4 L.

## How do you go from moles to liters?

Converting from moles to volume (liters): **Multiply your mole value by the molar volume constant**, 22.4L. Converting from particles (atoms, molecules, or formula units) to moles: Divide your particle value by Avogadro’s number, 6.02×10^{23}.

## How do you convert moles to gas?

Molar volume at STP can be used to convert from moles to gas volume and from gas volume to moles. The equality of **1mol=22.4L** is the basis for the conversion factor.

## Do gases occupy the same volume?

As all gases that are behaving ideally have the same number density, **they will all have the same molar volume**. At STP this will be 22.4 L. This is useful if you want to envision the distance between molecules in different samples.