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Assuming that water vapour is an ideal g...

Assuming that water vapour is an ideal gas, the internal energy change `(Delta U)` when `1 mol` of water is vapourised at `1` bar pressure and `100^(@)C`, (Given: Molar enthalpy of vapourization of water at `1` bar and `373K=41 kJ mol^(-1)` and `R=8.3J mol^(-1)K^(-1)`) will be:

A

`37.904kJmol^(-1)`

B

`41.00kJ mol^(-1)`

C

`4.100 kJ mol^(-1)`

D

`3.7904 mol^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
A
`Delta U=Delta H-Delta nRT`
`=41000-1xx8.314xx373=41000-3101.122`
`=37898.878J mol^(-1)=37.9 kJmol^(-1)`.
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