Calculate the change in entropy that occurs when 36.04 g of ice at –12.5°c is placed in 45.04 g of water at 100.0°c in a perfectly insulated vessel. assume that the molar heat capacities for and are 37.5 and 75.3 , respectively, and the molar enthalpy of fusion for ice is 6.01 kj/mol.

Entropy is defined as the measure of a system's thermal energy per unit temperature that is unavailable for doing work. The second law of thermodynamics states that the entropy of an isolated system never decreases over time

Explanation:

Entropy equal to change in mass divided by change in temperature

From above given M1 = 45.04g = 0.045kg

M2 = 35.04g = 0.036kg

T1 = -12.5oC, T2=100oC

Change in entropy of the system = (0.045 - 0.036)/ (100-(-12.5))

=0.009/112.5

=0.04

i believe the answer is true.