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)`)

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) )

What will be the volume of one mole of oxygen at 27^@C and at a pressure twice the standard atmosphere R=8.31 times 10^7 erg.mol^-1K^-1 .

At T K, what will be the value of (H-U) for 1 mol of ideal gas?

Show that the volume of 1 gram-molecule of any gas at 273K temperature and 1 atm pressure is 22.4 L.

The product of volume and pressure of how many gram of N_2 gas is 244 litre atmosphere at STP?

If the volume of air at 0^@C and 10 atmosphere pressure is 10 litre its volume in litre at normal temperature and pressure would be-

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

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

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)]