posted by kat on .
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
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.ºK)(4.0 mol)(273K-240K)
2. Melting of ice:
∆H2 = (4.0mol.)(5.0kJ/mol
3. Heating of water:
∆H3 = (74 J/mol.ºK)(4.0mol)(310ºK-273ºK)
Calculate and add the 3 enthalpies and add them up.
NOTE: 310 K is below the boiling of water. No significant evaporation takes place.