Why do real gases not behave exactly like ideal gases?

An ideal gas is a hypothetical gas consisting of identical particles of negligible volume, with no intermolecular forces. Also the atoms or molecules of the gas undergo perfectly elastic collisions with the walls of the container and each other. Real gases do not exhibit these exact properties.

because the particals will not move the same as real gases

answer; i believe that the correct answer is (c) explore the outer planets; / plz check good luck

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.