Answer:
160790 J
Explanation:
We can find the heat necessary for the ice to go from -20 degrees Celsius to 0 degrees Celsius:
[tex]Q=mc\Delta t[/tex]
Where [tex]c=2.09 J/g^{\circ}C[/tex] is the specific heat of ice, that is the amount of heat that must be supplied per unit mass to raise its temperature in a unit.
[tex]Q=(350g)(2.09 J/g^{\circ}C)(0^{\circ}C-(-20^{\circ}C))=14630 J[/tex]
We must calculate the latent heat of fusion required for this ice mass to change to water:
[tex]Q=mH[/tex]
Where H=334 J/g is the specific latent heat of fusion of water, that is the amount of energy needed per unit mass of a substance at its melting point to change from the solid to the liquid state.
[tex]Q=(350g)(334 J/g)=116900 J[/tex]
Then we calculate the heat necessary for the water to go from 0 degrees Celsius to 20 degrees Celsius:
[tex]Q=mc\Delta t[/tex]
Where [tex]c=4.18 J/g^{\circ}C[/tex] is the specific heat of water, that is the amount of heat that must be supplied per unit mass to raise its temperature in a unit.
[tex]Q=(350g)(4.18 J/g^{\circ}C)(20^{\circ}C-0^{\circ}C)=29260 J[/tex]
Finally the 3 results are added:
[tex]Q_{T}=14630 J + 116900 J + 29260 J=160790 J[/tex]
