Question

You place one mole of ice on a sidewalk. The outside temperature is30°C. As you
know, the ice will melt and the resulting liquid water will heatup. Assume the ice is initially at 0°C.
a. What is the change in the entropy of the system (i.e.H2O),
b. the surrounding, and
c. the universe for this process (ice melting + liquid heating)?(In reality, this process would also involve some waterevaporating. Ignore this effect). The molar heat capacity of liquidwater, CP(water) is 75.3 J/K/mol. Assume that CP(water) istemperature-independent. ?Hmelt (ice) = 6.02 kJ/mol at 0°C.