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Q.

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?

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a

48.6 kcal

b

52.23 kcal

c

44.87 kcal

d

56.06 kcal

answer is C.

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Detailed Solution

Change in enthalpy (∆H) = Heat of evaporation × Number of moles - 9.72 × 5ΔH=ΔE+ΔnRTΔE=48.6−5×2×10−3×373=44.87kcal
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