Calculate the work done when done when `1.0` mol of water at `373K` vaporises against an atmosheric pressure of `1.0atm`. Assume ideal gas behaviour.

Explanation

The volume occupied by water is very small and thus the volume change is equal to the volume occupied by `1g` mol of water vapour.
`V = (nRT)/(P) = (1.0 xx 0.0821xx 373)/(1.0) = 31.0L`
`W =- P_(ext) xx DeltaV =- (1.0) xx (3.10) L-atm`
`=- (3.10) xx 101.3J =- 3140.3J`