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 fullymolten 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 fullymolten 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 fullymolten sample of liquid at
660.4oC?
I found:
We possess:
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To calculate the total heat required, we need to consider two steps: heating the solid aluminum to its melting point and then melting it.

Heat required to raise the temperature of the solid aluminum: ( Q = m \times c \times \Delta T ) ( Q = 10.0 , \text{g} \times 0.89 , \text{J/g}^\circ \text{C} \times (660.4  580.0)^\circ \text{C} )

Heat required to melt the aluminum: ( Q = m \times \text{heat of fusion} ) ( Q = 10.0 , \text{g} \times 398 , \text{J/g} )
Total heat required: ( Q_{\text{total}} = Q_1 + Q_2 )
Calculate ( Q_1 ) and ( Q_2 ), then add them together to get ( Q_{\text{total}} ).
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