itfitzme
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- Jan 29, 2012
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The following are the succinct expressions of thermo. They apply to large bodies. A cup of water is large. The volume that can be observed in a microscope, where grains of pollen are visible, is not large enough.
Thermodynamics defines an ideal set of laws. Like all physics, it is difficult to so contol the environment as to create the ideal conditions. For instance, a thermous is very close to an isolated system, still it will lose heat.
The first law is;
-For an isolated system: ΔU=0
Energy is constant. Change in energy is zero
-For a non-isolated system: ΔU=Q-W
Change in internal energy is total heat minus work. Energy is conserved.
Adding heat increases energy. Doing work on the system increases energy. The direction, the minus sign is important. When a system does work, it loses energy.
A nice note is that friction is a form of work. Friction in an iaolated system is no change of energy to the system. The work done increases the heat without changing the energy. If automobile brakes were not cooled, they would get too hot. For a closed system the work done by the system and, typically, the heat is lost to the environment.
The 2nd law is;
-For a closex system ΔS>=0
Entropy increases to equilibrium
-For an open system dS= δQ/T
Change in entropy requires a change in heat and how much is required is inversely proportional to temperature.
Simple implications of first and second laws include
dU=T dS - δW
dU=T dS - p dV
These basically say that work may be extracted from the energy. But, in doing so, there are specific change to temperature and entropy. The direction of that change is apparent from the equations. Still, the context of the system is significant. The form does not guarantee that any particular system is suitable. For instance, right now I am hungry, so my entropy is low and less work is available.
The 3rd law is;
S(T→0)→0
At absolute zero temperature, entropy is zero.
At the very least, any understanding of thermo should include these. They are measurable. They are defined in specific contexts. Care should be taken to not over apply them, to not presume they imply things without clearly proving that they do.
Note that a virus is not large enough to be simply defined by the laws of thermodynamics presented here. It may or may not be true that these apply. One may not presume that they do as, by definition, a virus is below the size that is defined by thermodynamics.
Without extensive consideration, it is inapprooriate to apply the laws of thermodynamics to the origin of life except, perhaps, to note that the Earth was very hot at one time, increases temperature is higher entropy. High entroly means more ways that things may be arranged. As such, the instantaneous probability of life beginning was likely higher than now.
Thermodynamics defines an ideal set of laws. Like all physics, it is difficult to so contol the environment as to create the ideal conditions. For instance, a thermous is very close to an isolated system, still it will lose heat.
The first law is;
-For an isolated system: ΔU=0
Energy is constant. Change in energy is zero
-For a non-isolated system: ΔU=Q-W
Change in internal energy is total heat minus work. Energy is conserved.
Adding heat increases energy. Doing work on the system increases energy. The direction, the minus sign is important. When a system does work, it loses energy.
A nice note is that friction is a form of work. Friction in an iaolated system is no change of energy to the system. The work done increases the heat without changing the energy. If automobile brakes were not cooled, they would get too hot. For a closed system the work done by the system and, typically, the heat is lost to the environment.
The 2nd law is;
-For a closex system ΔS>=0
Entropy increases to equilibrium
-For an open system dS= δQ/T
Change in entropy requires a change in heat and how much is required is inversely proportional to temperature.
Simple implications of first and second laws include
dU=T dS - δW
dU=T dS - p dV
These basically say that work may be extracted from the energy. But, in doing so, there are specific change to temperature and entropy. The direction of that change is apparent from the equations. Still, the context of the system is significant. The form does not guarantee that any particular system is suitable. For instance, right now I am hungry, so my entropy is low and less work is available.
The 3rd law is;
S(T→0)→0
At absolute zero temperature, entropy is zero.
At the very least, any understanding of thermo should include these. They are measurable. They are defined in specific contexts. Care should be taken to not over apply them, to not presume they imply things without clearly proving that they do.
Note that a virus is not large enough to be simply defined by the laws of thermodynamics presented here. It may or may not be true that these apply. One may not presume that they do as, by definition, a virus is below the size that is defined by thermodynamics.
Without extensive consideration, it is inapprooriate to apply the laws of thermodynamics to the origin of life except, perhaps, to note that the Earth was very hot at one time, increases temperature is higher entropy. High entroly means more ways that things may be arranged. As such, the instantaneous probability of life beginning was likely higher than now.
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