A quantity of an ideal gas at `20^(@)C` reversibly expands against a constant pressure of 2.0 atm from 1.0 L to 2.0 L. Calculate the work done

A quantity of 4.0 moles of an ideal gas at 20^(@)C expands isothermally against a constant pressure of 2.0 atm from 1.0 L to 10.0L. What is the entropy change of the system (in cals)?

A quantity of 4.0 moles of an ideal gas at 20^(@)C expands isothermally against a constant pressure of 2.0 atm from 1.0 L to 10.0L. What is the entropy change of the system (in cals)?

A gas expands by 0.5L against a constant pressure of 1 atm . Calculate the work done in joule and calorie.

A gas expands by 0.5L against a constant pressure of 1 atm . Calculate the work done in joule and calorie.

An ideal gas is allowed to expand against a constant pressure of 2 bar from 10L to 50 L in one step. Calculate the amount of work done by the gas. If the same expansion were carried out reversibly, will the work done be higher or lower than the earlier case ? (Give that, 1 L bar = 100 J)

A gas expands 0.5 L against a constant pressure at 1 atm. Calculate the work done in joule and calorie.

A gas expands by 0.372 litre against a constant pressure of 1atm . Find the work done in cal.