Question

A 135g sample of ice is in a freezer at -21 degrees celsius. It is removed from the freezer and allowed to melt and the resulting water warms up to the room temperature of 23 degrees celsius. How much energy is absorbed by the 135g sample? The specific heat capacity of ice is 2.0J gC and the heat of fusion of ice is 0.33Kj g

m=135g
T1= -21C
T2= 23 C
c= 2.0J gC
H fusion = 0.33Kj g

Q=mcT
I don't know what to do after this

Answer 1

q1 = heat absorbed to move ice from -21 to zero C.
q1 = mass ice x specific heat ice x (Tfinal-Tinital)

q2 = heat needed to melt the ice; i.e., change solid ice @ zero C to liquid water @ zero C.
q2 = mass ice x heat fusion ice

q3 = heat needed to change T of water at zero C to 23 C.
q3 = mass water x specific heat water x (Tfinal-Tinitial)

Total Q = q1 + q2 + q3