Posted by **kat** on Sunday, February 1, 2009 at 9:00pm.

4 moles of water are heated from 240 K to 310. find delta entropy and graph entropy against K . Info : delta H fusion of water is 5 kJ/mol

delta H vaporization of water is 41.4 kJ/mol Cp of ice is 36 j/mol - k

Cp of water in liters is 74 j/mol-k

- chemistry -
**GK**, Monday, February 2, 2009 at 12:23am
From the information given, I think it is the enthalpy, ∆H, you need to find for the overall process.

You have the following calculations:

1. Heating of ice from 240 to 273 K:

∆H1 = (36 j/mol.ēK)(4.0 mol)(273K-240K)

2. Melting of ice:

∆H2 = (4.0mol.)(5.0kJ/mol

3. Heating of water:

∆H3 = (74 J/mol.ēK)(4.0mol)(310ēK-273ēK)

Calculate and add the 3 enthalpies and add them up.

NOTE: 310 K is below the boiling of water. No significant evaporation takes place.

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