H2(g)
and Cl2(g) are Kept in separate vessels of volume "V" at pressure "P"
and temperature "T" each. If suddenly pressure on both vessels are
doubled, which gas will occupy a greater volume.
If the walls of the vessels are rigid then both should occupy same volume since the meaning of volume of the gas generally implies volume of the container and not the sigma of the volume of the molecules/atoms.
This is actually my friends question and after giving him this reply , he gave his argument as follows:
I think sir, the idea you mentioned is applicable only to ideal gases. Coming to the case of real gases, doesn't the sizes of the molecules matter?
So he wants to know further sir.
I think sir, the idea you mentioned is applicable only to ideal gases. Coming to the case of real gases, doesn't the sizes of the molecules matter?
So he wants to know further sir.
volume of gas = volume of container in all cases ideal/real and the effect of the vol. of molecules is considered in the eq. of state not in the definition of vol.
For real gases,van der waal's equation will be valid.So,I think molecule which is greatre in size will have less effective volume to travel.