A gas expands isothermally from 1 litre to 10 litre at constant in internal energy of the system durin the opetation is

One mole of an ideal gas expands isothermally at 300 K from 1 litre to 101 litres at constant pressure of 1 atmosphere. The work done during this change is (1 lit atrn = 24.2 cals)

Two moles of an ideal gas is expanded isothermally and reversibly from 1 litre to 10 litre at 300 K. The internal energy change (in kJ) for the process (R = 8.3J)

Four moles of an ideal gas expand isothermally from 1 litre to 10 litres are 300 K. Calculated the change in free energy of the gas (R 8.314 JK^(-1)mol^(-1)) .

Four moles of an ideal gas expand isothermally from 1 litre to 10 litres are 300 K. Calculated the change in free energy of the gas (R 8.314 JK^(-1)mol^(-1)) .

" One mole of an ideal gas at "300K" is " , expanded isothermally from an initial , volume of 1 litre to 10 litres.The change , in internal energy for this process is : "(R=2 cal "mol^(-1)K^(-1)):" - "

A gas expands from 40 litres to 90 litres at a constant pressure of 8 atmosphers. Work done by the gas during the expansion is

Calculate the pressure-volume work by the system when the gas expands from 1.0 litre to 2.0 litre against a constant external pressure of 10 atmospheres. Express the answer in calorie and joule.

A gas expands from 10 litres to 20 litres against a constant external pressure of 10 atm. The pressure-volume work done by the system is

A gas expands from 10 litres to 20 litres against a constant external pressure of 10 atm. The pressure-volume work done by the system is