To produce silicon, used in semiconductors, from sand
\(\left(\mathrm{SiO}_{2}\right)\), a reaction is used that can be broken down
into three steps:
$$
\begin{aligned}
\mathrm{SiO}_{2}(s)+2 \mathrm{C}(s) \longrightarrow \mathrm{Si}(s)+2
\mathrm{CO}(g) & & \Delta H=689.9 \mathrm{~kJ} \\
\mathrm{Si}(s)+2 \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{SiCl}_{4}(g) & &
\Delta H=-657.0 \mathrm{~kJ} \\
\mathrm{SiCl}_{4}(g)+2 \mathrm{Mg}(s) \longrightarrow 2
\mathrm{MgCl}_{2}(s)+\mathrm{Si}(s) & & \Delta H=-625.6 \mathrm{~kJ}
\end{aligned}
$$
(a) Write the thermochemical equation for the overall reaction for the
formation of silicon from silicon dioxide; \(\mathrm{CO}\) and
\(\mathrm{MgCl}_{2}\) are byproducts.
(b) What is \(\Delta H\) for the formation of one mole of silicon?
(c) Is the overall reaction exothermic?