A closed, well-insulated container is filled with 454 g of water at 94.4 °C. To the hot water, 200 g of water ice at exactly 0 °C is added. The mixture reaches an equilibrium temperature of 41.1 °C. Assume the molar heat capacity is constant and all the processes are at constant pressure. The standard enthalpy of fusion for water at 0 °C is 6.008 kJ mol–1. The constant-pressure heat capacity for water is 75.291 J K–1 mol–1. Water has a molecular weight of 18.015 g mol–1. Calculate the entropy change (in J K–1) for the system that happened because of this mixing. I know the entropy change equals to q/t because q equals to the enthalpy exchange in the system as it is constant pressure, so what I did was: q=(454/18.015)75.291(41.1-94.4)+(200/18.015)75.291(41.1)+(200/18.015)*6008=172.2J change in entropy=172.2/(41.4+273)=0.55 Jk-1 That is apparently incorrect, what have I done wrong?