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Assuming that water vapour is an ideal g...

Assuming that water vapour is an ideal gas, the internal energy change `(DeltaU)` when 1 mol of water is vaporized at 1 bar pressure and `100^(@)`C, (given : molar enthalpy of vaporized of water of 1 bar and 373 K= 41 kJ `mol^(-1)` and `R = 8.314 JK^(-1) mol^(-1)` will beL

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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