Density of ideal gas at 2 atm and 600K is 2g/L. Calculate relative density of this with respect to Ne(g) under similar conditions : (given : `R=1/12 atm L/mol.K`)

Density of ideal gas of molecular mass 32 u at 1.2 atm pressure and 327 °C is

At 1 atm and 273 K the density of gas, whose molecular weight is 45, is:

2.8 g of a gas at 1atm and 273K occupies a volume of 2.24 litres. The gas can not be:

20g of ideal gas contains only atoms of S and O occupies 5.6 L at 1 atm and 273K. what is the molecular mass of gas ?

20g of ideal gas contains only atoms of S and O occupies 5.6 L at 1 atm and 273K. what is the molecular mass of gas ?

Calculate density of a gaseous mixture which consist of 3.01 xx 10^24 molecules of N_2 and 32 g of O_2 gas at 3 atm pressure and 860 K temperature (Given : R=1/12 atm L mol^(-1) K^(-1) )

1 mole of a ciatomic gas present in 10 L vessel at certain temperature exert a pressure of 0.96 atm. Under similar conditions an ideal gas exerted 1.0 atm pressure. If volume of gas molecule is negligible, then find the value of van der Waals' constant ''a'' (in atm L^(2)//mol^(2) ).

One mole of an ideal monoatomic gas at temperature T and volume 1L expands to 2L against a constant external pressure of one atm under adiabatic conditions, then final temperature of gas will be:

One mole of an ideal monoatomic gas at temperature T and volume 1L expands to 2L against a constant external pressure of one atm under adiabatic conditions, then final temperature of gas will be:

Two moles of an ideal gas at 1 atm are compressed to 2 atm at 273 K. The enthalpy change for the process is