Calculate the number of $kJ$ of heat necessary to raise the temperature of $60.0 \, g$ of aluminium from $35^{\circ} C$ to $55^{\circ} C$. Molar heat capacity of $Al$ is $24 \, J \, mol^{-1} \, K^{-1}$.

The heat required $(q)$ is given by the formula: $q = n \cdot C_m \cdot \Delta T$
First,calculate the number of moles $(n)$ of $Al$:
$n = \frac{\text{mass}}{\text{molar mass}} = \frac{60.0 \, g}{27.0 \, g \, mol^{-1}} = 2.222 \, mol$
Next,determine the change in temperature $(\Delta T)$:
$\Delta T = 55^{\circ} C - 35^{\circ} C = 20 \, K$
Now,substitute the values into the heat formula:
$q = 2.222 \, mol \times 24 \, J \, mol^{-1} \, K^{-1} \times 20 \, K$
$q = 1066.56 \, J$
Convert the heat to $kJ$:
$q = \frac{1066.56}{1000} \, kJ = 1.067 \, kJ$