Tenbears, I would say you have a lot right, along with a few misconceptions. Let me explain.
The "reaction" is due to the weak Van der Waals interaction between CO2 molecules and water molecules. This is the interaction that provides any driving force at all for the CO2 to be attracted to other molecules. But this is very weak; we are talking about meV (millielectron volts), not the eV (electron volts) scale characteristic of, say, covalent bonds.
You are certainly correct that the warming being discussed is not due to this exothermic reaction. (I am not sure that anyone actually asserted this.)
Due to this interaction, there is a slight propensity for the CO2 to be dissolved in water, rather than immediately being released. Thermal agitation provides enough energy to overcome this weak bonding, and to facilitate the CO2 leaving the wine. Because there are many more ways for the CO2 molecule NOT to be in the wine, the CO2 will leave until Henry's Law is satisfied.
(To help think about this, think about "dissolving" an H2O molecule in water; it has an attraction to other H2O molecules, which is why water is a liquid at room temperature. However, you may have noticed that water will evaporate at temperatures less than the boiling point. If air above the water is dry, there are many more ways for the H2O molecules to be in the air than in the water, so they preferentially evaporate until Henry's Law is satisfied, i.e., until the relative humidity is 100%.)
This is absolutely correct, and an important point. Henry's Law only describes the equilibrium situation.
But the statement above is a misconception. As I said above, the CO2 is held in the wine by the weak positive interaction with the water. It will leave the water, due to thermal agitation, until it is in equilibrium with the partial pressure of CO2 in the air above the water. It may take a long time to reach this equilibrium.
This is a misconception. Let me cite one fact that should allow you to see that your mental model of this process cannot explain all observed processes. The density of water is a maximum at 39F. As you cool water below 39F, it becomes less dense, i.e., it expands. And yet, the solubility of CO2 does not decrease under these circumstances; in fact, it increases.
That is correct. You got that part totally correct.
Are you serious? An exothermic reaction is a chemical or physical reaction that releases heat. It gives out energy to its surroundings. The energy needed for the reaction to occur is less that the energy it creates Where would the chemical reaction be? What chemicals are at work in this situation. What would be the physical reaction be? What energy is produced? The warming of wine is via convection and most certainly NOT by exothermic reaction.
The "reaction" is due to the weak Van der Waals interaction between CO2 molecules and water molecules. This is the interaction that provides any driving force at all for the CO2 to be attracted to other molecules. But this is very weak; we are talking about meV (millielectron volts), not the eV (electron volts) scale characteristic of, say, covalent bonds.
You are certainly correct that the warming being discussed is not due to this exothermic reaction. (I am not sure that anyone actually asserted this.)
Due to this interaction, there is a slight propensity for the CO2 to be dissolved in water, rather than immediately being released. Thermal agitation provides enough energy to overcome this weak bonding, and to facilitate the CO2 leaving the wine. Because there are many more ways for the CO2 molecule NOT to be in the wine, the CO2 will leave until Henry's Law is satisfied.
(To help think about this, think about "dissolving" an H2O molecule in water; it has an attraction to other H2O molecules, which is why water is a liquid at room temperature. However, you may have noticed that water will evaporate at temperatures less than the boiling point. If air above the water is dry, there are many more ways for the H2O molecules to be in the air than in the water, so they preferentially evaporate until Henry's Law is satisfied, i.e., until the relative humidity is 100%.)
Since the Co2 in the wine is introduced to it through an non atmospheric driving force it's partial pressure is not in equilibrium with atmospheric pressure but rather that of the driving force of its origin, (The fermentation process.)
This is absolutely correct, and an important point. Henry's Law only describes the equilibrium situation.
and is contained within the liquid in solution by atmospheric pressure, and the pressure exerted by the medium
But the statement above is a misconception. As I said above, the CO2 is held in the wine by the weak positive interaction with the water. It will leave the water, due to thermal agitation, until it is in equilibrium with the partial pressure of CO2 in the air above the water. It may take a long time to reach this equilibrium.
As the temperatures are reduced the molecules are constricted, creating a denser medium. The increased density of the medium has an inherent tendency to hold gas in solution because it has a sort of squeezing effect on the gas. Inversely as temperature increases nucleic action increases resulting in expansions of the molecules, creating a for lack of a better term looser medium. this decreased density allows, and in some cases forces the gas out of solution.
This is a misconception. Let me cite one fact that should allow you to see that your mental model of this process cannot explain all observed processes. The density of water is a maximum at 39F. As you cool water below 39F, it becomes less dense, i.e., it expands. And yet, the solubility of CO2 does not decrease under these circumstances; in fact, it increases.
Over a period of time the CO2 in solution within the wine dissipates in accordance with Henry's law since the air above it contains less than 1/10 of 1% co2 then the co2 in solution within that wine will be approximately 1/10 of 1%.
That is correct. You got that part totally correct.