
The theoretical lowest possible temperature, at which particles have minimal thermal motion.Absolute zero is the theoretical temperature at which a system has the minimum possible energy, corresponding to 0 K on the kelvin scale (-273.15 °C or -459.67 °F). At this temperature, particles have the smallest possible thermal motion, but they do not stop moving entirely: quantum mechanical zero-point energy remains. Absolute zero is a limit that can be approached but never exactly reached, according to the third law of thermodynamics. The pursuit of ever-lower temperatures has led to remarkable discoveries, such as superconductivity, superfluidity, and Bose-Einstein condensation.
The concept of absolute zero was first proposed by Guillaume Amontons in 1702, who noted that air pressure would vanish at a certain temperature. Lord Kelvin formalized the absolute temperature scale in 1848, and the third law of thermodynamics was formulated by Walther Nernst in 1906.
Reaching temperatures near absolute zero requires removing energy from a system. This is typically done using cryogenic techniques such as dilution refrigerators, which use a mixture of helium-3 and helium-4 to achieve temperatures below 0.1 K, or laser cooling, which uses photons to slow down atoms, reaching temperatures in the microkelvin range. The third law of thermodynamics states that as temperature approaches absolute zero, the entropy of a perfect crystal approaches zero, making it impossible to reach exactly 0 K in a finite number of steps.
Ultra-low temperatures are used in quantum computing to maintain the coherence of qubits, in precision measurements such as atomic clocks, and in the study of fundamental physics, including the search for dark matter.
In 2015, scientists at the University of Bremen achieved a temperature of 38 picokelvin (3.8 × 10^-11 K) in a gas of rubidium atoms, the coldest temperature ever recorded in a laboratory.
















