# Question #f0ab7

Feb 22, 2017

$3.96 \times {10}^{5} J$, rounded to two decimal places.

#### Explanation:

Taking Specific heat of Aluminum as $904 J {\left(k g K\right)}^{-} 1$

Heat required is given by
$\Delta Q = m s t$,
where $m , s \mathmr{and} t$ are the mass, specific heat and rise or gain in temperature of the object; and for change of state as
$\Delta Q = m L$
where $L$ is the latent heat for the change of state and
Total heat to be added is $\text{Heat required to raise the temperature of solid aluminum from "130^@C " to " 600^@C+"Heat required to melt it}$
$= m s t + m L$
$= 0.45 \times 904 \times \left(660 - 130\right) + 0.45 \times 4.0 \times {10}^{5}$
$= 215604 + 1.8 \times {10}^{5}$
$= 3.96 \times {10}^{5} J$, rounded to two decimal places.