An ideal gas has been placed in a tank at `37^@C`. The guage pressure is initially 609 kPa. One fourth of the gas is then released from the tank and thormal equilibrium is established. If the temperature is now `317^@`C, then the gauge pressure will be

When the pressure of a gas contained in a closed vessel is increased by 0.4% , the temperature increased by 1^@C . The initial temperature was :

A container of fixed volume 0.4 L contains 0.56 g of a gas at 27^(@)C . The pressure of the gas at this temperature is 936 mmHg. If the amount of the gas is increased to 2.1g and its temperature is decreased to 17^(@)C , then what will be the pressure of the gas? Assuming gas behaves ideally.

An ideal gas is heated from 27^@C to 627^@C at constant pressure. If initial volume was 3m^3 , then what will be the final volume ( in m^3 ) of gas?

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.

A vessel has nitrogen gas and water vapour in equilibrium with liquid water at a total pressure of 1 atm. The partial pressure of water vapours is 0.3 atm. The volume of this vessel is reduced to one third of the original volume, at the same temperature, then total pressure of the system is: (Neglect volume occupied by liquid water)

IF 2 mol of a gas at constant pressure, requires 70 cal heat to increase its temperature from 30^@C to 35^@C , then find its degrees of freedom.

Volume of a gas is doubled by raising its temperature at constant pressure . Initial temperature of the gas was 13^@C . Find the final temperature.

A gas is heated through 1^@C in a closed vessel and so the pressure increases by 0.4% . The initial temperature of the gas was