The reaction in which metal oxide is reduced by $\mathrm{Al}$is known as

We will perform many aluminothermic processes in this lab, which include oxidising aluminium ($\mathrm{Al}$) powder with a metal oxide $\left({\mathrm{M}}_{\mathrm{x}}{\mathrm{O}}_{\mathrm{y}}\right).$

$2\mathrm{Al}\left(\mathrm{s}\right)+\left(\frac{3}{y}\right){\mathrm{M}}_{\mathrm{x}}{\mathrm{O}}_{\mathrm{y}}\left(\mathrm{s}\right)⟶{\mathrm{Al}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)+3x\mathrm{M}\left(\mathrm{s}\right)$

In honour of their creator Hans Goldschmidt, these group of reactions is occasionally referred to as the Thermite Reaction or, more broadly, the Goldschmidt Reaction.

Typical oxidizers include ${\mathrm{Fe}}_2{\mathrm{O}}_3, {\mathrm{Cr}}_2{\mathrm{O}}_3$, and ${\mathrm{Mn}}_3{\mathrm{O}}_4$.

The tremendous exothermicity of these reactions makes them noteworthy.

Usually, the heat emitted is enough to turn the metal ($\mathrm{M}$) into a molten state.

The Heat of Formation of Aluminum Oxide plays a major role in the Goldschmidt Reaction.

$2\mathrm{Al}\left(\mathrm{s}\right)+\frac{3}{2}{\mathrm{O}}_2\left(\mathrm{g}\right)⟶{\mathrm{Al}}_2{\mathrm{O}}_3\left(\mathrm{s}\right){{\mathrm{\Delta H}}_{\mathrm{f}}}^{\circ }\left(298\right)=-1675.7\mathrm{kJ}/\mathrm{mol}$