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A reversible isothermal evaporation of 9...

A reversible isothermal evaporation of 90 g of water is carried out at `100^(@)C`. Heat of evaporation of water is 9.72 kcal `mol^(-1)`. Assuming water vapour to behave like an ideal gas, what is the change in internal energy of the system ?

A

48.6 kcal

B

52.23 kcal

C

44.87 kcal

D

56.06 kcal

Text Solution

Verified by Experts

Total Change in enthalpy `(Delta H) =` Heat of evaporation `xx` Number of moles `= 9.72xx5`
`Delta H = Delta E + Delta nRT`
`Delta E = 48.6-(5xx2xx10^(-3)xx373)=44.87 kcal R = cal K^(-1) mol^(-1)`
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