How much ice (in grams) would have to melt to lower the temperature of 355mL of water from 26∘C to 6∘C? (Assume the density of water is 1.0 g/mL.)

Answer 1

heat lost by ice + heat gained by melted ice + heat lost by water @ 20 cooling to 6 = 0

(x g ice x heat fusion) + [(x g melted ice x specific heat H2O x (Tfinal-Tinitial)] + [mass 20C H2O x specific heat H2O x (Tfinal-Tinitial)] = 0
Solve for x grams ice.
The answer I obtained is approx 80 g.

Answer 2

My solution assumes the the ice is at zero C.

Answer 3

355*4.18*(6-26)=-29678