(Answered) The equilibrium melting temperature of lead is 600 k and

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The equilibrium melting temperature of lead is 600 K and the latent heat of melting is Hm = 4810 Jmol. Calculate the change in molar enthalpy of lead when it solidifies spontaneously at a temperature of 550K and 1 atm pressure. Assume temperature independent heat capacities Cp = 28 J/K/mol for solid lead and Cp = 26 J/K/moll for liquid lead.

For the process of spontaneous solidification of lead described above, which are true:

Does the entropy of lead increase or decrease?

Does the total entropy of the "universe" increase, decrease or stay the same?

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