In a container, two moles of a diatomic ideal gas is allowed to expand against `1 atm` pressrue & volume change from `2` litre of `5` litre then calculate change in internal energy.

A gas absorbs 200J of heat and expands against the external pressure of 1.5 atm from a volume of 0.5 litre to 1.0 litre. Calculate the change in internal energy.

A gas of volume changes 2 litre to 10 litre at constant temperature 300K, then the change in internal energy will be :

A gas present at 5 atm pressure expands against one atmosphere when its volume changes from 3 litre to 5 litre. The work done by the gas in Joule will be ?

A gas occupies 2 litre at S.T.P. It is provided 300 joule heat so that its becomes 2.5 litre at 1 atm. Calculate change in its internal energy.

A gas occupies 2 litre at STP. It is provided 58.63 joule heat so that its volume becomes 2.5litre at 1 atm. Calculate change in its internal energy

Two moles of an ideal gas is expanded isothermally and reversibly from 2 litre to 20 litre at 300 K. The enthalpy change (in kJ) for the process is

5 mole of an ideal gas of volume is expanded against vaccum to make its volume 2 times, then work done by the gas is:

At 27^@C two moles of an ideal monatomic gas occupy a volume V. The gas expands adiabatically to a volume 2V . Calculate (a) final temperature of the gas (b) change in its internal energy and (c) the work done by the gas during the process. [ R=8.31J//mol-K ]

At 27^@C two moles of an ideal monatomic gas occupy a volume V. The gas expands adiabatically to a volume 2V . Calculate (a) final temperature of the gas (b) change in its internal energy and [ R=8.31J//mol-K ]

If two mole of an ideal gas at 546 K occupies a volume of 44.8 litres , the pressure must be :