its known that one mole of an ideal gas at STP(standard temperature and pressure)occupies 22.414dm3 volume?

Question

and
at STP distance between the melecules of an ideal gas is three hundered times greater than its diameter.(how its possible)
suppose diameter of h2 melecule is 2nm and two melecules are at a distance of 600nm.And diameter of CO melecule is 4nm(or take any other molecule larger in size than that of h2)and the distance between its two melecules will be 1200nm
so two melecules at STP are not occupying same volume.
if they have to occupy the same volume then CO molecules would have to come closer.
and if they come closer then distance between them will be not 300 times greater than their diameter.
if m wrong then how?

Answer 1

Who said that the intermolecular distance has to be 300 times greater than the diameter?
By definition an ideal gas has molecules of negligible volume which don't interact with each other. It is a hypothetical concept and in reality there are deviations depending on the chemical nature and size of the gas molecules and the conditions (pressure, temperature).

Answer 2

This constant volume of one mole of gas can be shown using classical physics (Newton's laws of motion mainly). So it applies to any set of small objects with kinetic energy.
STP is old stuff - now-a-days we use 298 K and 1 bar pressure and the volume of an ideal gas is .02479 m3 mol-1

Answer 3

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Answer 4

basically placed, it is because of the fact all suitable gases have an identical fee of R, the gas consistent. putting in the values for T, P, and n=a million will provide an identical fee whatever. Non-suitable (actual) gases will selection somewhat in the fee of R.