The theoretical concepts that underlie the Hot Ice experiment involve a supercooled, supersaturated aqueous solution becoming a solid. When a liquid is cooled beyond its freezing point but remains liquid is known as supercooling or undercooling, and being supersaturated occurs when the solutes in a solution exceed the saturation point. The sodium acetate in a supercooled state will rapidly change into a solid with the addition of physical energy or a nucleation site. During the transformation of the liquid supercooled solution into solid crystalline formation produces heat in an exothermic reaction, hence the name hot ice.
Enthalpy (ΔH) if negative indicates an exothermic reaction.
ΔH = energy used in bond breaking reactions − energy released
Enthalpy (ΔH) if negative indicates an exothermic reaction.
ΔH = energy used in bond breaking reactions − energy released