Question

Calculate the entropy change for the process of taking 1.00 kg of water from a temperature...

Calculate the entropy change for the process of taking 1.00 kg of water from a temperature of -26 C to +42 C keeping in mind that ice melts at 0 C. Assume a constant pressure of 1 bar and a temperature independent heat capacity within a given phase (Cpm = 37 J/Kmol for the solid and Cpm = 75 J/Kmol for the liquid state).

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Answer #1

as T= -26 0C = 273- 26 = 247 K and as T = 42 0C =42 + 273 K = 315K

S(1) = Cpm(H2O,solid) ln Tf/Ti =   37 J/Kmol ln 273K / 247K

= 37 J/Kmol ln 1.1052 = 37 * 0.10= 3.7 J/Kmol

S(2)= Cpm(H2O, liquid ) ln Tf/Ti = 75 J/Kmol ln 315K / 273K

= 75 J/Kmol  ln 1.1538 = =75 J/Kmol * 0.1430 = 10 .725J/Kmol

the change in entropy = S(1) + S(2) =  3.7 J/Kmol +10 .725J/Kmol = + 14.425 J/Kmol

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