Calculate`q, W, DeltaU` and `DeltaH` for the isothermal reversible expansion of one mole of an ideal gas from an initial pressure of `1.0` bar to a final pressure of `0.1` bar at a constant temperature of `273K.`

Explanation

In isothermal process as temperature remains constant both `DeltaU` and `DeltaH` are zero.
`DeltaU=0,Deltah=0`
Applying first law of thermodynamics,
`DeltaU=w+Q`
`0=w+Q`
or `Q=-w=-2.303nRT" "log((P_(1))/(P_(2)))`
`=2.303xx1xx8.314xx273" log "((1)/(0.1))`
`=5227.169J=5.227kJ`