The final volume (in L ) of one mole of an ideal gas initially at `27^(@)C` and 8.21 atm pressure,if it absorbs 420 cal of heat during a reversible isothermal expansion is (ln2=0.7)

One mole of an ideal gas at 27^(@) ,8.21 atm absorbs 420 cal of heat during a reversible isothermal expansion. Calculate the final volume (in litre) of gas. [Use: R=0.0821 " litre-atm"//"K-mole"]

One litre of an ideal gas st 27^(@)C is heated at a constant pressure to the 297^(@)C. Then, the final volume is the approximately

Two moles of an ideal gas at 2 atm and 27^(@)C is compressed isothermally to half of its volume by external pressure of 4 atm. The work doen is

4 moles of an ideal gas is at 0^(@) C . At constant pressure it is heated to double its volume, then its final temperature will be

Two moles of an ideal gas initially at 27^(@)C and one atmospheric pressure are compressed isothermally and reversibly till the final pressure of the gas is 10 atm calculate q, w and Deltaw for the process

In an isothermal expansion of one mole of an ideal gas against vacuum from 10 litre to 100 litre at 27^(@)C , the quantity of heat absorbed by the gas is

Calculate q,w , and DeltaU for the isothermal reversible expansion of one mole of an ideal gas from an initial pressure of 2.0 bar to a final pressure of 0.2 bar at a constant temperature of 273K .