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An adiabatic process is a thermodynamic process, there is no gain or loss of heat.
Josianne Prohaska
Wiki User
∙ 9y agoAn adiabat is the curve on a graph of pressure and temperature which indicates the adiabatic heating or cooling of a gas - that is, which attains no change in entropy.
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Is it possible to get to 0 kelvin?
It may be reachable somewhere in the universe far from any outside forces but we'll never witness it. I don't care who says otherwise... we will never witness it. You couldn't even record it without causing the temperature to raise. Any source of light, motion, etc would keep whatever it is you're trying to examine from reaching zero kelvin. What would happen is all theory. I can't give any 100% true answers for that. I'm not a big fan of a lot of the scientific theories floating around out there.
Does molecular motion ever stop?
At a molecular level, molecules will always vibrate to some degree. This vibration causes what is known as Brownian motion and molecular vibrations cause bumps and collisions against other molecules which result in random motion, much like how vibrators may bounce of one another when in contact and vibrating. Why molecules will always vibrate is due to the laws of thermodynamics. Only at absolute zero (0 K) will a molecule cease to vibrate. However, absolute zero can never be achieved artificially, though it is possible to reach temperatures close to it through the use of cryocoolers. This is the same principle that ensures no machine can be 100% efficient. Laser cooling is another technique used to take temperatures to within a billionth of a degree of 0 K. At temperatures near 0 K, nearly all molecular motion ceases and ΔS = 0 for any adiabatic process. Pure substances can (ideally) form perfect crystals as Temperature approaches 0. Max Planck's strong form of the third law of thermodynamics states the entropy of a perfect crystal vanishes at absolute zero. The original Nernst heat theorem makes the weaker and less controversial claim that the entropy change for any isothermal process approaches zero as Temperature approaches 0. The implication is that the entropy of a perfect crystal simply approaches a constant value. The Nernst postulate identifies the isotherm T = 0 as coincident with the adiabat S = 0, although other isotherms and adiabats are distinct. As no two adiabats intersect, no other adiabat can intersect the T = 0 isotherm. Consequently no adiabatic process initiated at nonzero temperature can lead to zero temperature. In other words, it is impossible by any procedure to reduce the temperature of a system to zero in a finite number of operations. Therefore molecules will alwyas be moving due to the impossibility to drive the temperature down to 0 K, which if it were possible would stop movement entirely.
Is it possible to get to 0 kelvin?
It may be reachable somewhere in the universe far from any outside forces but we'll never witness it. I don't care who says otherwise... we will never witness it. You couldn't even record it without causing the temperature to raise. Any source of light, motion, etc would keep whatever it is you're trying to examine from reaching zero kelvin. What would happen is all theory. I can't give any 100% true answers for that. I'm not a big fan of a lot of the scientific theories floating around out there.
What this car is?
I assume you mean how do you achieve absolute zero temperature, so here it is:Absolute zero is the theoretical temperature at which entropy reaches its minimum value. The laws of thermodynamics state that absolute zero cannot be reached using only thermodynamic means.A system at absolute zero still possesses quantum mechanical zero-point energy, the energy of its ground state. The kinetic energy of the ground state cannot be removed. However, in the classical interpretation it is zero and the thermal energy of matter vanishes.The zero point of any thermodynamic temperature scale, such as Kelvin or Rankine, is set at absolute zero. By international agreement, absolute zero is defined as 0K on the Kelvin scale and as −273.15 °C on the Celsius scale.[1][2] This equates to −459.67 °F on the Fahrenheit scale and 0 °R on the Rankine scale.[2] Scientists have achieved temperatures very close to absolute zero, where matter exhibits quantum effects such as superconductivity and superfluidity.At temperatures near 0 K, nearly all molecular motion ceases and, when entropy = S, ΔS = 0 for any adiabatic process. Pure substances can (ideally) form perfect crystals as T → 0. Max Planck's strong form of the third law of thermodynamics states the entropy of a perfect crystal vanishes at absolute zero. The original Nernst heat theorem makes the weaker and less controversial claim that the entropy change for any isothermal process approaches zero as T → 0:The implication is that the entropy of a perfect crystal simply approaches a constant value.The Nernst postulate identifies the isotherm T = 0 as coincident with the adiabat S = 0, although other isotherms and adiabats are distinct. As no two adiabats intersect, no other adiabat can intersect the T = 0 isotherm. Consequently no adiabatic process initiated at nonzero temperature can lead to zero temperature. (≈ Callen, pp. 189-190)-Courtesy of Wikipedia.org
Does molecular motion ever stop?
At a molecular level, molecules will always vibrate to some degree. This vibration causes what is known as Brownian motion and molecular vibrations cause bumps and collisions against other molecules which result in random motion, much like how vibrators may bounce of one another when in contact and vibrating. Why molecules will always vibrate is due to the laws of thermodynamics. Only at absolute zero (0 K) will a molecule cease to vibrate. However, absolute zero can never be achieved artificially, though it is possible to reach temperatures close to it through the use of cryocoolers. This is the same principle that ensures no machine can be 100% efficient. Laser cooling is another technique used to take temperatures to within a billionth of a degree of 0 K. At temperatures near 0 K, nearly all molecular motion ceases and ΔS = 0 for any adiabatic process. Pure substances can (ideally) form perfect crystals as Temperature approaches 0. Max Planck's strong form of the third law of thermodynamics states the entropy of a perfect crystal vanishes at absolute zero. The original Nernst heat theorem makes the weaker and less controversial claim that the entropy change for any isothermal process approaches zero as Temperature approaches 0. The implication is that the entropy of a perfect crystal simply approaches a constant value. The Nernst postulate identifies the isotherm T = 0 as coincident with the adiabat S = 0, although other isotherms and adiabats are distinct. As no two adiabats intersect, no other adiabat can intersect the T = 0 isotherm. Consequently no adiabatic process initiated at nonzero temperature can lead to zero temperature. In other words, it is impossible by any procedure to reduce the temperature of a system to zero in a finite number of operations. Therefore molecules will alwyas be moving due to the impossibility to drive the temperature down to 0 K, which if it were possible would stop movement entirely.
