What is the change in entropy of `1.00 mol` of liquid water at `0.0^@ C` that freezes to ice at `0.0^@ C` ?

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We can use the definition of entropy change to find the change in entropy of the liquid water as it freezes.

The change of entropy of the water is given by:


Where the heat removed from the water is `Q_(rem)` .

`Q_(rem)` is also a product of the latent heat of fusion and its mass.


Where `n` is the number of moles and `M` is the molar mass.


`DeltaS=Q_(rem)/T=(-nML_f)/T=(-(1.00 mol)(18.015 g/(mol))(333.5 J/g))/(273 K)=-22.0 J/K`

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