Posted by Katrina on .
A 13.0-g sample of ice at -13.0°C is mixed with 112.0 g of water at 80.0°C. Calculate the final temperature of the mixture assuming no heat loss to the surroundings. The heat capacities of H2O(s) and H2O(l) are 2.08 and 4.18 J/g · °C, respectively, and the enthalpy of fusion for ice is 6.02 kJ/mol.
(heat to move ice from -13 to 0) + heat to melt ice) + (heat to move melted ice from 0 to final) + (heat lost by 112 g H2O @ 80) = 0
[(mass ice x specific heat ice x (0-(-13))] + [mass ice x heat fusio] + [mass melted ice x specific heat water x (Tfinal-Tinitial)] + (mass water x specific heat water x (Tfinal-Tinitial)] = 0
Solve for Tfinal. Answer is close to 63 C.