Question

Two kg of ice melts at 0 degree C at constant atmospheric pressure and changed

to form liquid water at 25 degree C. If the latent heat of fusion of ice is 333.3 kJ/kg,

calculate the entropy change during process.
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Answer 1

Total heat = Heat required to convert 2kg of ice to 2kg of water at 0℃ +Heat required to convert 2kg of water at 0℃ to 2kg of water at 20℃

Heat=mhfg+mCp\Delta t$$

Here, m(mass of ice)=2kg

hfg(latent heat of fusion of ice)=334kJ

Cp of water(specific heat)=4.187 kJ/kg-k

Δt(temperature difference) =20℃

Therefore,

Heat required=2×334+2×4.187×(20−0)

=835.48 kJ

Therefore, to melt 2kg of ice 835.48kJ of heat is required.

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