Home
Class 11
CHEMISTRY
A weighed quantity of a gas is collected...

A weighed quantity of a gas is collected over water at `25^(@)C` and 742 mmHg. The molar mass of the gas is to be determined at standard temperature and pressure. If the vapor pressure of water is ignored during the calculation, what is the effect on the calculated pressure and calculated molar mass of the gas?

Promotional Banner

Similar Questions

Explore conceptually related problems

calculate the molar mass of the water.

Molar heat capacity of a gas at constant temperature and pressure is:

The density of a gas was found to be 2.92gl^-1 at 27^@C and 2.0 atm. Calculate the molar mass of the gas.

135 mL of a gas is collected over water at 25^(@)C and 0.993 bar. If the gas weighs 0.160 g and the aqueous tension at 25^(@)C is 0.0317bar, calculate the molar mass of the gas.

750 mL of nitrogen are collected over water at 25^@C and 740 mm pressure. If the aqueous tension at this temperature is 23.8 mm Hg, calculate the mass of the dry gas.

A 50mL sample of gas is collected over water. What will be the effect on the calculated molar mass of the gas if the effect of the water vapour is ignored? It will be:

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.

A certain quantity of a gas occupied 50 ml, when collected over water at 15^@C and 750 mm pressure. If the dry gas occupies 45.95 mL at NTP, calculate the aqueous tension at 15^@C .