As a subject matter expert in thermodynamics and physics, I can provide an informed perspective on the concept of absolute zero and its attainability.

Absolute zero is a theoretical temperature limit that represents the point at which the kinetic energy of particles in a substance is at its minimum. It is defined as 0 Kelvin (-273.15 degrees Celsius or -459.67 degrees Fahrenheit). At this temperature, particles are theoretically supposed to have no kinetic energy, and thus, no thermal motion.

In practice, reaching absolute zero is considered impossible due to the Third Law of Thermodynamics, which states that the entropy of a perfect crystal approaches zero as the temperature approaches absolute zero. Entropy is a measure of the randomness or disorder of particles in a system. The Third Law implies that as you get closer to absolute zero, it becomes increasingly difficult to remove additional entropy from the system.

Furthermore, the concept of quantum mechanics also comes into play. Quantum mechanics introduces the idea of quantum fluctuations, which are random, spontaneous changes in energy at very low temperatures. These fluctuations mean that particles cannot ever be completely still, even at absolute zero.

In conclusion, while absolute zero is a well-defined concept in thermodynamics, achieving it is not possible due to the fundamental laws of physics and the principles of quantum mechanics.

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Absolute zero is often thought to be the coldest temperature possible. ... At the physically impossible-to-reach temperature of zero kelvin, or minus 459.67 degrees Fahrenheit (minus 273.15 degrees Celsius), atoms would stop moving. As such, nothing can be colder than absolute zero on the Kelvin scale.read more >>