At `25^(@)C`, a 0.01 mole sample of a gas is compressed from 4.0 L to 1.0 L at constant temperature. What is the work done for this process if the external pressure is 4.0 bar?

Temperature of one mole of a gas is increased by 1^(@) C at constant pressure. The work done on the system is

One mole of an ideal gas at 25^(@)C expands in volume from 1.0 L to 4.0 L at constant temperature. What work (in J) is done if the gas expands against vacuum (P_("external") = 0) ?

A gas expands from 4.0 L to 4.5 L against a constant external pressure of 1 atm. The work done by the gas is (1 L-atm = 101.3 J)

5.6 liter of helium gas at STP is adiabatically compressed to 0.7 liter. Taking the initial temperature to be T_1, the work done in the process is

5.6 liter of helium gas at STP is adiabatically compressed to 0.7 liter. Taking the initial temperature to be T_1, the work done in the process is

One mole of a gas is heated at constant pressure to raise its temperature by 1^(@)C . The work done in joules is

One mole of an ideal gas is expanded from a volume of 3L to 5L under a constant pressure of 1 atm. Calculate the work done by the gas.

A sample of a gas occupies 650.0 cm at 100^@C . At what temperature the gas will occupy a volume of 1050.0 cm^3 if the pressure is kept constant ?

Temperature of 1 mole of a gas is increased by 2^(@)C at constant pressure. Work done is :

The temperature of n-moles of an ideal gas is increased from T_0 to 2T_0 through a process p=alpha/T . Find work done in this process.