Posted by Jessica on .
Two 20.0-g ice cubes at –20.0 °C are placed into 295 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature of the water after all the ice melts.
Heat capacity of H2O(s)=37.7J
Heat capacity of H2O(l)=75.3J
Enthalpy of fusion of H2)=6.01kJ
heat to raise 40 g ice from -20 to zero.
q1 = mass x specific heat x (Tfinal-Tinitial)
heat to melt 40 g ice.
q2 = mass ice x heat fusion (in joules)
heat to raise melted water to final T.
q3 = mass water x specific liquid water x (Tfinal-Tinitial)
heat absorbed by 295 g H2O @ 25.0C
q4 = mass H2O x specific heat liquid H2O x (Tfinal-Tinitial).
q1 + q2 + q3 + q4 = 0
Substitute and solve for Tfinal. Watch the signs.