4 moles of a van dr Walls'gas is subjected to 3 Kj of hrat in a closed rigid vessel of volume 20.2 L causing an increase in temperature from 300 K to 400 K. Calculate the value of `DeltaH` (inJ) for the above change
[Given data : `R=0.08 L` bar `"mole"^(-)K^(-1),a=2 L^(2)` bar `mol^(-2),b=0.05L"mole"^(-1)`]

Some amount of diatomic van der walls' gas is kept in a rigid container of volume 20 liter and subjected to change in temperature from 300 K to 400 K. If 30 kacl of heat is required and enthalpy change of the process is observed to be (310)/(9) kacl, then estimate the number of moles of the gas. [Given : b=0.1 L mol^(-1) , a= 1.25 atm -L^(2)//mol^(2) ]

Calculate work done when 1 mole of an ideal gas is expanded reversibly from 20 L to 40 L at a constant temperature of 300 K.

10 moles of an ideal gas confined to a volume of 10 L is released into atmosphere at 300 K where the pressure is 1 bar. The work done by the gas is: ltBrgt (R=0.083L" bar "K^(-1)mol^(-1))

Calculate the pressure of 154 g carbon dioxide in a vessel of 2.0 L capacity at 30^(@)C , a = 648 L bar atm K^(-1) mol^(-1), b = 0.0427 L mol^(-1)

Calculate the pressure of 154 g carbon dioxide in a vessel of 2.0 L capacity at 30^(@)C , a = 648 L bar atm K^(-1) mol^(-1), b = 0.0427 L mol^(-1)

Two moles of an ideal gas is expanded isothermally and reversibly from 1L to 10 L at 300 K. The enthalpy change (in kJ) for the process is

Two moles of an ideal gas is expanded isothermally and reversible from 1 L to 10 L at 300 K. The enthalpy change (in kJ) for the process is

When 5 moles of an ideal gas is expanded at 350 K reversibly from 5 L to 40 L, then the entropy change for the process is (R = 2 cal mol^(-1) K^(-1))