The large amount of heat evolved in displacement reactions is significant because it can cause the metals involved to be produced in the molten state.

Displacement reactions involving highly reactive metals and metal compounds are highly exothermic because a large amount of heat is released during the reaction.

The process of obtaining metals from their compounds involves reduction, where metal oxides are reduced to their elemental form. This process is a chemical reaction involving the transfer of electrons, which is characteristic of reduction reactions.

Highly reactive metals function as reducing agents by displacing metals of lower reactivity from their compounds through displacement reactions. They donate electrons to the metal ions, causing them to be reduced to their elemental form.

Some examples of highly reactive metals used as reducing agents include sodium, calcium, and aluminium.