34.05 mL of phosphorus vapour weighs 0.0625g at `546^@C` and 0.1 bar pressure .what is the molar mass of phosphorus ?

Density of a gas at 30^(@)C and 1.3 atm pressure is 0.027 g*mL^(-1) . What is the molar mass of the gas?

. 3.7 g of a gas at 25^@C occupied the same volume as 0.184 g of hydrogen at 17^@C and at the same pressure. What is the molar mass of the gas ?

2.9 g of a gas at 95^(@)C occupied the samme volume as 0.184 g of dhydrogen at 17^(@)C , at the same pressure, what is the molar mass of the gas?

The volume of 0.44 g of a colourless oxide of N_(2) is 224 mL at 273^(@)C and 1530 mm pressure. What is the compound?

A vessel of 120 mL capacity contains amount of gas at 35@C and 1.2bar pressure. The gas is transferred to another vessel of volume 180 mL at 35^@ . What would be its pressure ?

A vessel of 120 mL capacity contains a certain amount of gas at 35^(@)C and 1.2 bar pressure. The gas is transferred to another vessel of volume 180 mL at 35^(@)C . What would be its pressure ?

Analysis of a compound of phosphorous shows that 1.0 litre of it at STP never contains less than 1.384 g of the' element,Again 1.0 litre phosphorous vapour at STP weighs 5.536 g. Calculate approximate atomic mass, molecular mass and atomicity.

At 25^(@)C and at a certain pressure, 3.7 g of a gas occupies the same volume as the volume occupied by 0.184 of H_(2) gas at 17^(@)C and the same pressure. Calculate molar mass of the gas.

The vapour pressure of pure benzene at a certain temperature is 0.850 bar. A non-volatile, non-electrolyte solid weighing 0.5 g when added to 39.0 g of benzene (molar mass 78 g mol^-1 ), vapour pressure of the solution, then, is 0.845 bar. What is the moler mass of the solid substance ?

1.19g of volatile liquid gas on complete vaporisation gives 216ml of its vapour at 27^(@) and 755 mm pressure. Calculate molar mass of liquid. (R=0.082litatmK^(-)mol^(-))