Two moles of an ideal gas is expanded isothermally and irreversibly at `27^(@)C` from volume `V_(1)" to" 2.5 V_(1)"and" 4.17KJ` heat is absorbed from surroundings. Determine `DeltaS_("sys")`?

Two moles of an ideal gas is expanded irreversibly and isothermally at 37^(@)C until its volume is doubled and 3.41 KJ heat is absorbed from surrounding. DeltaS_("total")("system +surrounding") is:

Three moles of an ideal gas are expanded isothermally and reversibly at 27^(@)C to twice its original volume. Calculate q, w, and DeltaU .

2 mol of an ideal gas at 27^(@) C expand isothermally and reversibly from a volume of 2L to 20L. The work done (in KJ) by the gas is :-

Two moles of helium gas expanded isothermally and irreversibly at 27^(@)C from volume 1 dm^(3) to 1 m^(3) at constant pressure of 100 k Pa. Calculate the work done.

Two moles of an ideal gas expanded isothermally and reversibly from 1L to 10L at 300K . What is the enthalpy change?

5mol of an ideal gas at 27^(@)C expands isothermally and reversibly from a volume of 6L to 60L . The work done in kJ is

5mol of an ideal gas at 27^(@)C expands isothermally and reversibly from a volume of 6L to 60L . The work done in kJ is

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

If x mole of ideal gas at 27^(@)C expands isothermally and reversibly from a volume of y to 10 y, then the work done is

6mole of an ideal gas expand isothermally and reversibly from a volume of 1 litre to a volume of 10 litre at 27° C .The maximum work is done