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)`

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)

A 2L flask contains 0.4 g O_(2) and 0.6 g H_(2) at 100^(@)C . Calculate the total pressure of the gas mixture in the flask.

At 100^(@)C a 2 litre flask contains 0.4 g of O_(2) and 0.6 g of H_(2) . What is the total pressure of this gas mixture in the flask?

In a 10 litre volumetric flask contains 1 gram He and 6.4 and gram O_2 at 27^@C temperature If that total pressure of the mixture is 1.107 atmosphere then what is the partial pressure of He and O_2 ?

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) )

Calculate the total number of electrons present in 1.4 g of dinitrogen gas.

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) )

Calculate the osmotic pressure of a 10%. Solution of glucose at 18^@C . R = 0.082 lit 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) ]

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)]