A sample of phosphorus that weighs `12.4g` exerts a pressure 8 atm in a `0.821` litre closed vesel at `527^@ C`. The molecular formula of the phosphorus vapour is :

2g of H_2 and 17g of NH_3 are placed in a 8.21 litre flask at 27^@C . The total pressure of the gas mixture is?

240 mL of a dry gas measured at 27°C and 750 mm pressure weighed 0.64 g. What is the molecular mass of the gas ?

34.05 mL of phosphorus vapours weighs 0.0625 g at 546^(@)C and 0.1 bar pressure. What is the molar mass of phosphorus ?

9.00 litres of a gas at 16 atm and 27°C weigh 93.6 g. What is the molecular mass of the gas ?

When 3.2 g S is vaporized at 450^(@)C and 723 mm pressure, the vapours occupy a volume of 780 mL What is the molecular formula of S vapours ?

8.2 L of an ideal gas weights 9.0 g at 300 K and 1 atm pressure. The molecular mass of the gas is

A duma bulb full of air weighs 22.567 gm at 20^@C and 755 mm pressure. Full of vapours of a substance at 120^@C and the same pressure. It weighs 22.8617 gm. The capacity of the bulb is 200 ml. Find out the molecular mass of the substance. [density of air =0.00129(gm)/(ml) ]

A sample of charcoal weighing 6 g was brought into contact with a gas contained in a vessel of one litre capacity at 27^(@)C . The pressure of the gas was found to fall from 700 to 400 mm. Calculate the volume of the gas (reduced to STP) that is adsorbent under the condition of the experiment ("density of charcoal sample is" 1.5 g cm^(3)) .

Find the no. of mole of phosphorus in 92.9 g of phosphorus assuming that molecular formula of phosphorus in P_(4^(.) . Also determine the no. of atoms and molecules of phosphorus in the sample.

34.05 mL of phosphorus vapours weighs 0.0625 g at 546^(@)C and 0.1 bar pressure. What is the molar mass of phossphorus ?