In which temperature 14 gm `N_2` at 1.642 atm pressure occupies 10 lt?
[R = 0.0821 L atm//mol^(-K)`]

At 273 K and 76 cm pressure, the volume of 0.64 g of any gas is 224 mL. At what temperature 1 g of that gas at 1 atm pressure will occupy a volume of 1 litre?

A gas of molar mass 84.5 g//mol is enclosed in a flask at 27^@C has a pressure of 2 atm. Calculate the density of the gas. [R = 0.082 L atm K^(-1) mol^(-1)]

At constant temperature and 1 atm pressure, an ideal gas occupies a volume of 3.25m^(3) . Calculate the final presure of the gas in the units of atm, torr and Pa if the its volume is reduced to 1.25m^(3) while its temperature is kept constant.

What is meant by the molarity of a solution ? What would be the osmotic pressure of a 0.02 molar aqueous solution of urea at 27^(@)C ? (R = 0.082 L.atm.K^(-1). Mol^(-1) )

At a certain temperature, 1 mol of chlorine gas at 1.2 atm takes 40 sec to diffuse while 1 mol of its oxide at 2 atm takes 26.5 sec. the oxide is-

A gas of molar mass 84.5g/mol is enclosed in a flask at 27^(@)C has a pressure of 2 atm. Calculate the density of the gas. [R=0.082 *atm*K^(-1)*mol^(-1) ]

At a temperature of 273K and 1 atm pressure 1L of a gas weighs 2.054g. Calculate its molecular mass.

Calculate (1) the enthalpy change in the fusion of 100 g ice at 0^(@)C temperature and 1 atm pressure pressure (2) the enthalpy change in the vaporisation of 10g water at 100^(@)C temperature and 1 atm pressure. Givenn : Latent heat of ice at 0^(@)C temperature and 1 atm pressure =6.02kJ*mol^(-1) and latent heat of vaporisation of water at 100^(@)C temperature= 40.4kJ*mol^(-1) .

A sample of gas at 0^@C and 1.00 atm pressure occupies 3.00 L. What change in temperature in @C is necessary to adjust the pressure of that gas to 1.5 atm after it has been transferred.to a 2.00 L container ?