The apparent contradiction is.. A box containing two gases (N2 & 02) at equal temperature and pressure separated by a partition. When the partition is removed the original state of ORDER moves to a more DISORDERED state driven by the second law towards equilibrium of position. The entropy (IF entropy = measure of disorder) clearly increases BUT the heat equation ds = dQ/T = 0..!! What's going on.. simple ds = dQ/T is NOT a complete statement of entropy change. It only accounts for the natural tendency to equilibrium of MOMENTUM.. but not equilibrium of POSITION.. Both are required, its just that equilibrium of position is not often required in the measure so we don't need it. dQ/T makes thermodynamic calculations of entropy based on macro properties like pressure and temperature possible.
What is happening is the random motion of atoms causes any system to move to a state which more probable among all its other possible states. It does this simply because there are many more ways of being in disordered state than an ordered state. This is what Boltzmann's equation is all about.
(absolute entropy) s = k.log(W) so entropy change ds = s2 - s1
hence ds = k.log (W2) - k.log(W1) = k.log(W2/W1)
Now W2/W1 = (final #num of microstates)/(initial #num of microstates)
So if we are dealing cards for instance..
A royal flush (RF) is an ordered state = low entropy
There are 7 RF's per suit so 28 per deck = (28 microstates)
There are 52C7 possible hands = 133784560 (microstates)
So W2/W1 = 28/133784560 BUT that = Probability of (RF)..
So the actual entropy change of dealing RF is
ds = k.log(Pr(RF))
It does not matter that we are only calculating ds for card dealing and not the cards themselves.. Not only does this tell us..
Entropy = Measure of Disorder.. it also gives meaning to the term..
Order = Improbability..
It is utterly false to say entropy is not a measure of disorder. By Appendix 5.1 of [The God Law] we may also say to pay the entropy cost of dealing a royal flush from a well shuffled deck is 1/Pr(RF)) = dealing 4.778 million hands (that's on average).
Thursday, 28 April 2016
Sunday, 24 April 2016
4.4 LIES
In the previous box example it is important you understand how we place our system boundaries to calculate the entropy change. If we put a boundary around the surface of the hot body as the heat is lost to the surroundings the temperature will be seen to drop from 200 C to 100 C.. The average being 150 C. The change in entropy (hot body) is then very roughly given by..
ds = Integral{dQ/T} (Integral = Sum of [dQ1/T1 + dQ2/T2 + dQ3/T3 ... ]
~= Q/Taverage)
ds(hot) ~= -Q/150 (-ve for heat out) and for the cold body Taverage = 50 C
ds(cold) ~= Q/50 (+ve heat in)
So ds(total) = Q/50 - Q/150 = Q(3-1)/150 = Q/75 +ve increase.
Note inside the box (closed system) we have two sub-systems each with an OPEN boundary to their surroundings.. The effect of heat flow out of the hot body decreases entropy of the system and the reverse is true for the cold body but they are not equal and the sum is always greater than zero. Establishing for every entropy decrease there must be a greater increase in the surroundings caused by that decrease which gives us the Second Law.
If we now cyclically open the ends of the box first allowing the suns radiant heat to fall on the hot end then cold of space on right end indefinitely you have both entropy drop and increase in open systems powered by the sun working in accordance with the second law. Just like the Earth.
According to evolutionists that's all there is to it.. but is it.
Lets now replace the hot and cold bodies with Nitrogen and Oxygen gasses separated by the same partition but with both at the same temperature and pressure. When we open the partition the gasses will mix by diffusion but no heat is transferred and so..
ds = Integral{dQ/T} = 0 (No change in entropy for whole box)
But the initial separation of gasses is a state of order which the diffusion process, on removing the partition, will destroy. The uniformly mixed gasses will not separate by themselves because it is an irreversible increase in entropy.. All in accordance with the second law..!
ds = Integral{dQ/T} (Integral = Sum of [dQ1/T1 + dQ2/T2 + dQ3/T3 ... ]
~= Q/Taverage)
ds(hot) ~= -Q/150 (-ve for heat out) and for the cold body Taverage = 50 C
ds(cold) ~= Q/50 (+ve heat in)
So ds(total) = Q/50 - Q/150 = Q(3-1)/150 = Q/75 +ve increase.
Note inside the box (closed system) we have two sub-systems each with an OPEN boundary to their surroundings.. The effect of heat flow out of the hot body decreases entropy of the system and the reverse is true for the cold body but they are not equal and the sum is always greater than zero. Establishing for every entropy decrease there must be a greater increase in the surroundings caused by that decrease which gives us the Second Law.
If we now cyclically open the ends of the box first allowing the suns radiant heat to fall on the hot end then cold of space on right end indefinitely you have both entropy drop and increase in open systems powered by the sun working in accordance with the second law. Just like the Earth.
According to evolutionists that's all there is to it.. but is it.
Lets now replace the hot and cold bodies with Nitrogen and Oxygen gasses separated by the same partition but with both at the same temperature and pressure. When we open the partition the gasses will mix by diffusion but no heat is transferred and so..
ds = Integral{dQ/T} = 0 (No change in entropy for whole box)
But the initial separation of gasses is a state of order which the diffusion process, on removing the partition, will destroy. The uniformly mixed gasses will not separate by themselves because it is an irreversible increase in entropy.. All in accordance with the second law..!
Tuesday, 12 April 2016
4.3 LIES
I have had some very strange comments about what is 'design' so that comes up next.. But first we must get the thermodynamics straight.. Let us start with an approximately CLOSED SYSTEM. As in all experimental work.. there are no perfectly closed systems but we can approximate one and get the calculations to work quite well.. Consider a well insulated box with a removable partition.. Hot mass left.. Cold mass to right..
{ [ 200 deg ] | [ 0 deg ] } => { [ 190 deg ] Q=> [ 10 deg ] }..
which becomes { [ 100 deg ] [ 100 deg ] } for equal masses..
When we remove the insulated partition a quantity of heat Q will flow from left to right until the temperatures of the two masses are equal and there it will remain.. which is called equilibrium. After which we will never observe either side become hot while the other gets cool because it would violate the 2nd Law of thermodynamics.. even though this is physically possible.! Why.. its just too improbable. Which establishes the true basis of the 2nd Law.. probability. Heat or any form of energy 'flows' because there are more ways energy can be spread out than be gathered together. We can simply state the 2nd Law as (it used to be stated until recent confusion set in)..
All systems of particles left to themselves will tend to move to their most probable state..
The law is also stated as "entropy always increases in an isolated system". If we now define entropy from this probabilistic basis as a measure of disorder, this immediately gives us a definition of ORDER = IMPROBABLE.. Hot on one side and cold on the other is an ordered state of matter.. The 2nd Law simply says systems left to themselves tend to disorder.. So you may ask where are the lies..?
The lies are to be found here.. [http://www.talkorigins.org/faqs/thermo/entropy.html] the atheist propaganda page.. Where they assert..
"But what of entropy and disorder? Where does that identification fit into the structure of thermodynamics? The answer is, nowhere. It is not an axiom or first principle, it is not derived from any other basic principles, and nowhere is it required or even used at all to do any of the science to which thermodynamics applies. It is simply irrelevant and out of place except as an interesting aside."
While correct to say the concept of entropy as a measure of disorder is not used in practical thermodynamics it is incorrect to say "It is not an axiom or first principle" it most definitely is. The simple reason its not used is Boltzmann's equation for absolute entropy based solely on the probability of a state of matter existing can't be calculated. We would have to know the momentum and position of every atom in the system.! So how is it relevant..?
{ [ 200 deg ] | [ 0 deg ] } => { [ 190 deg ] Q=> [ 10 deg ] }..
which becomes { [ 100 deg ] [ 100 deg ] } for equal masses..
When we remove the insulated partition a quantity of heat Q will flow from left to right until the temperatures of the two masses are equal and there it will remain.. which is called equilibrium. After which we will never observe either side become hot while the other gets cool because it would violate the 2nd Law of thermodynamics.. even though this is physically possible.! Why.. its just too improbable. Which establishes the true basis of the 2nd Law.. probability. Heat or any form of energy 'flows' because there are more ways energy can be spread out than be gathered together. We can simply state the 2nd Law as (it used to be stated until recent confusion set in)..
All systems of particles left to themselves will tend to move to their most probable state..
The law is also stated as "entropy always increases in an isolated system". If we now define entropy from this probabilistic basis as a measure of disorder, this immediately gives us a definition of ORDER = IMPROBABLE.. Hot on one side and cold on the other is an ordered state of matter.. The 2nd Law simply says systems left to themselves tend to disorder.. So you may ask where are the lies..?
The lies are to be found here.. [http://www.talkorigins.org/faqs/thermo/entropy.html] the atheist propaganda page.. Where they assert..
"But what of entropy and disorder? Where does that identification fit into the structure of thermodynamics? The answer is, nowhere. It is not an axiom or first principle, it is not derived from any other basic principles, and nowhere is it required or even used at all to do any of the science to which thermodynamics applies. It is simply irrelevant and out of place except as an interesting aside."
While correct to say the concept of entropy as a measure of disorder is not used in practical thermodynamics it is incorrect to say "It is not an axiom or first principle" it most definitely is. The simple reason its not used is Boltzmann's equation for absolute entropy based solely on the probability of a state of matter existing can't be calculated. We would have to know the momentum and position of every atom in the system.! So how is it relevant..?
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