Find volume of 2 moles of a vander waals gas at critical pressure & critical temperature. Given for gas : `[P_(C)=2atm and T_(C)=300K]`

The volume of 0.5 mole of gas at 1 atm pressure and 273^(@)C temperature is

The Boyle temperature of a van der Waal gas is -246^(@)C . Its critical temperature on absolute temperature scale is :

Volume of 0.5 mole of a gas at 1 atm. Pressure and 273 K is

Consider the following statements. If the Van der Waal's parameters of two gases are given as :- {:(, a//dm^(6) "bar mol"^(-2), b//dmmol ^(-1)), (Gas A , 6.5, 0.055), (Gas B , 2, 0.01):} (i) Critical volume of A lt Critical volume of B (ii) Critical pressure of A gt Critical pressure of B (iii) Critical temperature of A gt Critical temperature of B Which of the above statements is/are incorrect?

Calculate the volume occupied by 2 moles of an ideal gas at 2.5xx10^(5)Nm^(-2) pressure and 300K temperature.

The internal pressure loss of one mole of vander Waal gas over an ideal gas is equal to