Question

# 1. At the normal melting point of ice ∆Hfus= 6.007 kJ mol−1 and ∆Sfus= 22.00 J...

1. At the normal melting point of ice ∆Hfus= 6.007 kJ mol−1 and ∆Sfus= 22.00 J K−1 mol−1.
a) What is ∆Gfusat the normal melting point? Look at your answer. Is it correct? Why or why not?

b) Determine ∆G for freezing water at 1 atm and -10oC assuming that ∆Hfusand ∆Sfusdo not change much over the 0 → −10oC temperature range.

c) Determine ∆G for freezing water at 1 atm and -10oC assuming that ∆Hfusdoes not change much over the 0 → −10oC range.

a)

Melting point of ice is T= 273.15K

So

The answer is wrong as should be zero at 273.15K as at that temperature there is an equilibrium between ice and water.

b) At T=273.15-10=263.15K ,

c) Entropy change is given by .

so if the molar specific heat at constant pressure cp is given then we can find the and thus find as done in part b.

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