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

Volume of 0.5 mole of a gas at 1 atm. pressure and 273^@C is

Volume of 1.5 mole of a gas at 1 atm. pressure and 273K is

Calculate the moles of an ideal gas at pressure 2 atm and volume 1 L at a temperature of 97.5 K

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

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

Figure, shows the variation of potential energy (U) of 2 mol of Argon gas with its density in a cyclic process ABCA . The gas was initiallly in the state A whose pressure and temperature are P_(A)=2 atm, T_(A)=300K , respectively. It is also stated the path AB is a rectangular hyperbola and the internal energy of the gas at state C is 3000r . Based on the above information answer the following question : The heat supplied to the gas in the process AB is

The temperature of 5 moles of a gas is decreased by 2K at constant pressure of 1 atm. Indicate the correct statement

1mol of an ideal gas at 400K and 10atm is allowed to expand, adiabatically, against 2.0atm external pressure. Find the final temperature of the gas. [Use: C_(v) = (5)/(2)R]

The essential conditions for liquefaction of gases were discovered by Andrews in 1869 as a result of his study of pressure-volume-temperature relationship for CO_(2) . It was found that above a certain temperature, it was impossible to liquefy a gas whatever the pressure was applied. The temperature below which the gas can be liquefied by the application of pressure alone is called critical temperature (Tc). The pressure required to liquefy a gas at this temperature is called the critical pressure (Pc). The volume occupied by one mole of the substance at the critical temperature and pressure is called critical volume. Critical constants are related with van der waals' constant as follows: V_( c) = 3b, P_( c) =a/(27b^(2)), T_( c) =(8a)/(27 Rb) The values of critical volumes of four gases A, B, C and D are 0.025L, 0.312L, 0.245L and 0.432L respectively. The gas with larger molecular diameter will be :

Calculate van der Waals constansts a and b if critical temperature and critical pressure are 30^(@)C and 72 atm respectively .