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Assuming that water vapour is an ideal gas, the internal energy change ΔU() when 1 mol of water is vaporised at 1 bar pressure and 100° C, (Given : Molar enthalpy of vaporization of water at 1 bar and 373K=41kJmolmol1 and  R=8.3Jmol1K1 )  will be: 

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a
37.904 kJ mol1
b
41.00 kJ mol1
c
4.100 kJ mol1
d
3.7904 kJ mol1

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detailed solution

Correct option is A

Here ,the change in internal energy,

ΔU=ΔHΔngRT;ΔU=411×8.3×3731000=37.904kJ/mol

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