Compute the entropy difference between 12 kg of water at 40°C and 12kg of ice at -10°C.
Heat of melting of ice=336 kJ/kg
Standard entropy of water at 298K = 69.9 J/K.mol
S=the integral of cp/TdT
The Attempt at a Solution
I broke it down into different phases, the first one being delta S from -10 to 0, then from 0 to 40 degrees. Then I will add the heat of melting to the total entropy. Mass should be irrelevant since it remains constant. My problem is what to do with the standard entropy of water. Am I supposed to add it to my entropy equaiton as well?