Pressure of 1 g of an ideal gas A at `27^@C` is found to be 2 bar when 2g of another ideal gas B is introduce in the same flask at same temperature the pressure becomes 3 bar. Find a relationship between their molecular masses.

Pressure of 1g of ann ideal gas A at 27^(@)C is found to be 2 bar. When 2 g of another ideal gas B is introduced in the same flask at same temperature, the pressure becomes 3 bar. Find a relationship between their molecular masses.

When 2 g of a gas 'M' is introduced into an empty flask at 30^(@)C , its pressure becomes 1 atm. Now, if 3g of another gas 'N' is introduced in the same flask at the same temperature, the total pressure becomes 1.5 atm. Find the ratio of the molar masses of the two gases.

When a flask of fixed volume is filled with (x)/(2) mol of an ideal gas A at a constant temperature, the pressure of the gas becomes 2 atom. Adint 2 y mol of another ideal gas B to the flask at the same temperature causes the pressure of the system to increase to 4.0 atm.

At a temperature of 273K and 1 atm pressure 1L of a gas weighs 2.054g. Calculate its molecular mass.

The pressure of 3 mol of an ideal gas is 10 atm at 27^(@)C . Calculate work done by the gas when it is expanded isothermally against an external pressure of 1 atm.

Volume of a given mass of an ideal gas is VL at 27^(@)C and 1 atm pressure. If volume of the gas is reduced by 80% at constant pressure, temperature of the gas will have the be-

The pressure exerted by 12 g of an ideal gas at temperature t^@C in a vessel of volume V litre is one atm.when the temperature is increased by 10 degree at the same volume.the pressure increases by 10% calculate the temperature t and volume v.(molecular weight of the gas =120).

At a given temperature and pressure, the volume of 1 mol of an ideal gas is 10 L. at the same temperature and pressure, the volume of 1 mol of a real gas is VL. At this temperature and pressure, if the compressibility factor of the real gas is greater than 1, then -

Pressure exerted by 12g of an ideal gas at t^(@)C in a vessel of volume VL is 1 atm. When the temperature is increased by 10^(@)C at the same volume, the pressure increased by 10% . Calculate the temperature 't' and volume V (molar mass of gas=120).

. 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 ?