A 5.0 litres cylinder contained 10 moles of hydrogen gas at 27°C. Due to leakage, entire gas escaped into the atmosphere. The atmospheric pressure is 1.0 atm. Calculate the work done by the gas assuming hydrogen to be an ideal gas.

Explanation

Initial volume of the gas = 0.5 L
Since, hydrogen is assumed to behave as an ideal gas, the final volume is given by
`V = (nRT)/P = (10 xx 0.0821 xx 300)/(1.0) = 246.3 L`
`:. Delta V = 246.3 - 5.0 = 241.3 L`
Hence, W = - `P DeltaV`
` = - 1 xx (241.3) L` atm
` = - 241.3 xx 101.3 J ( :. 1 L a t m = 101.3 J)`
`=24443.7 J`
` = 24.4 kJ`