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)]`

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) ]

Calculate the osmotic pressure of a 10%. Solution of glucose at 18^@C . R = 0.082 lit atm K^-1 mol^-1 .

Density of a gas at -135^(@)C and 50.66 atm pressure is 2g*cm^(-3) . What is the density of the gas at STP?

1 g of a gas at 7^@C and 2 atmosphere pressure occupies a volume of 410 ml. Determine the molar mass of the gas. (R = 0.082 litre atmosphere mole^(-1) K^(-1) )

2 mol of a van der waals gas at 27^(@)C occupies a volume of 20 L. what is the pressure of the gas? [a=6.5 atm*L^(-2)*mol^(-2),b=0.056L*mol^(-1) ]

1.19g of volatile liquid gas on complete vaporisation gives 216ml of its vapour at 27^(@) and 755 mm pressure. Calculate molar mass of liquid. (R=0.082litatmK^(-)mol^(-))

Calculate the total pressure in a 10 L cylinder which contains 0.4 g of helium, 1.6 g of oxygen and 1.4 g of nitrogen at 27^(@) C. Also calculate the partial pressures of He gas in the cylinder. Assume Ideal behaviour for gases. R = 0.082 L atm k^(-1) mol^(-1)

The weight of 350 mL of a diatomic gas at 0^(@)C temperature and 2 atm pressure is 1g. Calculate the weight of its one atom.

Density of a gas at 30^(@)C and 1.3 atm pressure is 0.027 g*mL^(-1) . What is the molar mass of the gas?

The number of molecules 67.2 L of a gas at 0^@C and 1 atm pressure is: