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Absolute Zero

Absolute zero is defined as the point where no more heat can be removed from a system, according to the absolute or thermodynamic temperature scale.

This corresponds to 0K (zero degrees Kelvin), or - 273.15 oC, or - 459.67 F.

In terms of the Kinetic Theory Absolute Zero happens when all movement of individual molecules stops. However, experimental evidence indicates this isn't the case - it indicates that particles at absolute zero do have minimal motion - but there is still some vibration. So, while heat may not be removed from a system at absolute zero, absolute zero does not represent the lowest possible enthalpy state.

In quantum mechanics, absolute zero represents the lowest internal energy of solid matter in its ground state.

The temperature of an object depends on the speed at which its atoms and molecules move - rotate, translate or oscillate. Absolute Zero represents only oscillations at their slowest speed - motion never completely stops. But it has not proved to be possible, thus far, to reach absolute zero—though scientists have approached it. The National Institute of Standards and Technology (NIST) achieved a record cold temperature of 700 nK (billionths of a kelvin) in 1994. Massachusetts Institute of Technology researchers set a new record of 0.45 nK in 2003.