One problem that we have here is that we have not all defined exactly what we are talking about. One thing that has yet to be well enough defined in entropy.Originally posted by Phillip:
UTEOTW, even this example surprises me. You seem much smarter than this. The "order" is already set by the physical shape of the molecules, the molecules have no choice but to settle together in six pointed shapes simply because of their shape.
All that has exchanged by lowering the temperature is removing the energy that causes those initially shaped molecules jostling around.
This is a very sad example of entropy increase, and you complain about the YEC people trying to come up with a hypothesis that fits their theory. You are doing no better with THIS particular example. See if you can give a better example.
Now, entropy is a property of something just like temperature or pressure is. It is specific, it has units. Now one difference between temperature and entropy is that you can measure temperature directly while you cannot do the same for entropy. But for entropy, unlike temperature, only the change is important. Let's give an example of another such property that may be easier to understand.
There is a property call enthalpy. Now this is more directly related to what people think of as energy. It, too, cannot be measured directly. So, for water let's say, we define a specific set of conditions (temperature, pressure,...) and define the enthalpy to be a certain value. From there we can calculate or measure changes and know what the enthalpy of water is at any other set of conditions. We even make it easy and put these into tables. So if you want to know how much heat it takes to heat water at atmospheric pressure from 100F to 200F you just look those points up on the chart and subtract the values.
Now, the same thing happens with entropy. It is a property of the water and we define the value at a certain point and set all the other values relative to that. The charts I mentioned earlier (steam tables) will often include the entropy data. For an example go to this page
http://www.engineersedge.com/thermodynamics/steam_tables.htm
and look at the chart at the bottom of the page.
So, back to the ice. When we say that the entropy of the water decreased when it froze, we are talking about a very real property of the water. We can even calculate the value specifically.
The latent heat of fusion of water is 144 Btu/lb. Let's say that the outside temperature is 20F and you are taking one pound of water at 32F to ice at 32 F. The formula is deltaS = Q / deltaT
So, the decrease in entropy of the water is 144 / (32+460) = 0.293
The increase of entropy of the air is 144 / (20+460) = 0.3
So you see that the entropy of the water decreased. Also note that the entropy of the air increased more than the decrease of the water. This process followed thermodynamics and resulted in a decrease in the entropy of the water accompanied by a net increase in the entropy of the universe. It was spontaneous. No one had to force anything. The water went to a higher ordered state spontaneously.
That is why this is a good example. It shows how locally increased order and lower entropy can come about spontaneously. It is something which everyone can understand. To get into chemistry and how some reactions can be favored while others are not favored is much harder to see. To take that further and talk about equilibrium constants and how even the unfavored reaction can proceed to some extent gets deeper. To then apply this concept to life which does not operate at equilibrium conditions becomes even more complex. To then try and explain how the non-equilibrium conditions means that entropy is actually a driving force TOWARDS life, well most people are lost at that point.
But ice, hey, most people can understand that.