. 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?

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.

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?

At STP, 0.44 g of a gas has the volume of 224 cm^(3) . What is the molecular mass of the gas?

10 g of solute A and 20 g of solute B both are dissolved in 500 mL of water. The solution has the same osmotic pressure as 6.67 g of A and 30 g of B are dissolved in the same volume of water at the same temperature. What is the ratio of molar masses of A and B ?

The density of CO_(2) at STP is 1.96g*L^(-1) . A sample of CO_(2) occupies a volume of 480 mL at 17^(@)C and 800 mm Hg pressure. What is the mass of the sample?

0.0286g of a gas at 25^(@)C and 76 cm presure occupies a volume of 50cm^(3) . What is molarr mass of the gas?

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

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 -135^(@)C and 50.66 atm pressure is 2g*cm^(-3) . What is the density of the gas at STP?