Home
Class 11
CHEMISTRY
The mass of 525 ml of a gaseous compound...

The mass of 525 ml of a gaseous compound at `28^(@)C` and 0.970 bar pressure was found to be 0.900 g. Calculate the molar mass of the compound.

Text Solution

AI Generated Solution

To calculate the molar mass of the gaseous compound, we can use the ideal gas equation, which is given by: \[ PV = nRT \] Where: - \( P \) = pressure (in bar) - \( V \) = volume (in liters) - \( n \) = number of moles ...
Promotional Banner

Topper's Solved these Questions

  • STATES OF MATTER : GASES AND LIQUIDS

    MODERN PUBLICATION|Exercise Practice Problems|54 Videos

  • STATES OF MATTER : GASES AND LIQUIDS

    MODERN PUBLICATION|Exercise Advanced Level (PROBLEMS)|14 Videos

  • SOME BASIC CONCEPTS OF CHEMISTRY

    MODERN PUBLICATION|Exercise COMPETITION FILE (INTEGER TYPE AND NUMERICAL VALUE TYPE QUESTIONS)|10 Videos

  • STRUCTURE OF ATOM

    MODERN PUBLICATION|Exercise Unit Practice Test|13 Videos

Similar Questions

Explore conceptually related problems

The mass of 525 cm^(3) of a gaseous compound at 28^(@)C and 730 torr was found to be 0.900 g. Calculate the molar mass of the compound.

Calculate the number of moles of hydrogen contained in 18 litres of a gas at 27^(@)C and 0.92 bar pressure. If the mass of hydrogen is found to be 1.350g . Calculate the molecular mass of hydogen.

The density of a gas is found to be 1.56 g dm^(-3) at 0.98 bar pressure and 65^(@)C . Calculate the molar mass of the gas.

The density of a gas at 27^(@)C and 1 bar pressure is "2.56 g L"^(-1) . Calculate the molar mass.

The mass of 500 mL of hydrogen gas at a pressure of 1 bar and at temperature of 300 K was found to be 4.09xx10^(-2)g . Calculate the molar mass of hydrogen.

Calculate the mass of 0.120 dm^(3) of N_(2) at 150^(@)C and 0.987 bar pressure.

The mass of 0.5 dm^(3) of hydrogen at a pressure of 1 bar of Hg and at a temperature of 300 K was found to be 4.0 xx 10^(-2) g . Calculate the molar mass of hydrogen.

If the osmotic pressure of 5g per litre solution of compound at 27^(@)C is 0.025 atm, calculate the molecular mass of the compound.

A given mass of gas occupies 919.0 mL of dry state at N.T.P. The mass when collect over water at 15^(@)C and 0.987 "bar" pressure occupies one litre volume. Calculate the vapour pressure of water at 15^(@)C .