10 moles of a liquid L are 50% converted into its vapour at its boiling point `(273^@C)` and at a pressure of 1 atm.If the value of latent heat of vap
10 moles of a liquid L are 50% converted into its vapour at its boiling point `(273^@C)` and at a pressure of 1 atm.If the value of latent heat of vapourisation of liquid L is 273 L atm/mole , than which of the following statements is/are correct : Assume volume of liquid to be negligible and vapour of the liquid to behave ideally.
A. Work done by the system in the above process is 224 L atm
B. The enthalpy change `(DeltaH)` for the above process is 1365 L atm (with respect to magnitude only)
C. The entropy of the system increases by 2.5 L atm in the above process
D. The value of `DeltaU` for the above process is 1589 L atm.
1 Answers
Correct Answer - ABC
`V_f=5xxRxx546=224 L`
`W=-P_(ext)(DeltaV)=-1` atm (224 L) =-224 L atm
`:.` work done by system =224 L atm
Enthalpy change `(DeltaH)=q=273xx5=1365 L atm`
`DeltaS=(DeltaH_(vap))/T=1365/546=2.5` L atm /K
`DeltaU=q+W=1365-224=1141 L atm`