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## Main Question or Discussion Point

so i have been trying to calculate boltsmann constant by assuming the fact that for an ideal gas the equation :

PV=nRT is true.

i assume that for containing each molecule the wall needs to apply a force. now here is where it get's a little weird.

each molocule should be only deflected in the direction that the wall is hitting it and so each molecule hits all walls (expect the one that exactly moves parallel to the wall) and each one has effect on the pressure.

but from what i see in books, my way only works, if i assume that each molecule gets deflected exactly in opposite of it's own direction, so only one third of the molecules interact with the selected wall.

my question is that is there any sort of "evidence" that shows proves the constant multiplications of the relation between boltsmann constant and average kinetic energy of a molecule in an ideal gas which is

E=(3/2)kT ?

is there any evidence for that (3/2) or it's just purely theoretical?

PV=nRT is true.

i assume that for containing each molecule the wall needs to apply a force. now here is where it get's a little weird.

each molocule should be only deflected in the direction that the wall is hitting it and so each molecule hits all walls (expect the one that exactly moves parallel to the wall) and each one has effect on the pressure.

but from what i see in books, my way only works, if i assume that each molecule gets deflected exactly in opposite of it's own direction, so only one third of the molecules interact with the selected wall.

my question is that is there any sort of "evidence" that shows proves the constant multiplications of the relation between boltsmann constant and average kinetic energy of a molecule in an ideal gas which is

E=(3/2)kT ?

is there any evidence for that (3/2) or it's just purely theoretical?