Calculate the volume occupied by `8.8` g of `CO_(2)` at `31.1^(@)C` and 1 bar pressure `(R=0.083 "bar" LK^(-1) "mol"^(-1))`

Calculate the temperature of 14 mol of a gas occupying 10 dn^(3) at 3.32 bar pressure ( R=0*083 bar dm^(3)"mol"^(-1)K^(-1))

What is the molar mass of a gas whose density is 1.5 g L^(-1) at 27^(@)C and 1 atm pressure ? (Use R = 0.08L atm mol^(-1) K^(-1) )

Calculate the pressure in a mixture of 8g of O_(2)(g) and 4 g of H_(2)(g) confined in a vessel of 1 dm^(3) "at" 27^(@)C (R=0*083 dm^(3) "bar" K^(-1) "mol"^(-1))

3 gram of non-volatile solute in a 1000 cm^(3) of water shows an osmotic pressure of 2 bar at 300K. Calculate the molar mass of the solute (R=0.0853" L bar "K^(-1)mol^(-1)) .

The osmotic pressure of a solution was found to be 8 atm when 8 mol of a non-volatile solute was dissolved in V L of solution at 300 K .Calculate the volume of solution (R=0.0821 L-"atm" K^(-1) "mol"^(-1))

Molar volume is the volume occupied by 1 mol of any (ideal) gas at standard temperature and pressure (STP : 1 atmospheric pressure, 0^circ C) i.e.,

Volume occupied by one molecule of water (density = 1 g cm^-3 ) is :

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)