Question

Calculate the total heat (in Joules) needed to convert 1.602 x 101 grams of ice at -1.383oC to liquid water at 8.554 x 101oC.
Melting point at 1 atm 0.0oC
Cwater(s) = 2.09 J/goC
Cwater(l) = 4.18 J/goC
delta Hofus = 6.02 kJ/mol

Answer 1

q1 = heat needed to raise T of solid ice at -1.383 to zero C.
q1 = mass ice x specific heat ice x (Tfinal-Tinitial)

q2 = heat needed to melt ice; i.e., change phase from solid to liquid.
q2 = mass ice x heat fusion

q3 = heat needed to raise T of liquid water from zero C to 85.54 C.
q3 = mass water x specific heat H2O x (Final-Tinitial)

Total: add q1 + q2 + q3.