Question

Solid aluminum has a specific heat of 0.89 J/g oC, and a heat of fusion of 398 J/g. Aluminum melts at 660.4oC. How much heat is required to convert a 10.0 g sample of aluminum metal at 580.0oC to a fully-molten sample of liquid at 660.4oC?

Solid aluminum has a specific heat of 0.89 J/g oC, and a heat of fusion
of 398 J/g. Aluminum melts at 660.4oC. How much heat is required to convert a
10.0 g sample of aluminum metal at 580.0oC to a fully-molten sample of liquid at
660.4oC?

Answer 1

I found: `4695.6J`

Explanation:

Here you have a bloc of solid aluminium and you heat it up to reach the temperature of fusion and then you supply a bit more of heat to completely melt it.
So in total you have:
`Q_1+Q_2=`
Where:

`Q_1=mc_"Al"DeltaT` is the heat needed to heat up your bloc from `580^@C` to `660.4^@C`

`Q_2=mL_f` is the heat needed not to increase its temperature but to melt it completely.

We have:

`Q_1+Q_2=mc_"Al"DeltaT+mL_f=`

`=10*0.89*(660.4-580)+10*398=4695.6J`