Vanderwaal's constant in litre atmosphere per mole for carbon dioxide are a = 3.6 and b = `4.28 xx 10^(-2)`. Calculate the critical temperature and critical volume of the gas. R = 0.0820 lit atm `K^(-1). Mol^(-1)`

Vanderwaal's constants for hydrogen chloride gas are a = 3.67 atm lit^(-2) and b = 40.8 ml mol^(-1) . Find the critical temperature and critical pressure of the gas.

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

Calculate the temperature of 4.0 moles of a gas occupying 5dm^3 at 3.32 ber. (R = 0.083 bar dm^3K^(-1)mol^(-1)

Calculate the temperature of 4.0 mol of gas occupying 5 dm^(3) at 3.32 bar. (R=0.083 bar *dm^(3)*K^(-1)*mol^(-1) )

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)]

Calculate the total pressure in a 10 litre cylinder which contains 0.4 g He, 1.6 g O_2 and 1.4 g N_2 at 27^@C . Also calculate the partial pressure of Helium gas in the cylinder. Assume ideal behaviour of gas (R=0.082 litre-atm K^(-1)mol^(-1)

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) )

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) ]

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

What will be the volume of 8g of H_2 gas (H = 1) at the pressure of atmosphere and temperature of 300K? (R = 0.082 litre-atmosphere mol^(-1)K^(-1) )