Is it possible, in a simple way, to reduce the amount of gas that escapes from a Coke bottle?
While the bottle is closed, the gas inside the liquid is in equilibrium with the gas in the bottle.Equilibrium does not mean that there are no gases leaving the liquid, but that the amount of gas leaving is exactly equal to the amount entering back. This can be understood if you see the system of the liquid and the gas as one big system. There is no reason for there to be more gas in the gas phase than in the liquid. This state would be thermodynamically unstable. That is why concentrations will be compared by venting the gas into the air. The second law of thermodynamics explains that every system strives to increase its entropy level, or decrease the amount of order in it. A large gas density in one place in the system and a small one in another defines a state of excessive order. By mixing the gas homogeneously, the concentration is equalized. When we open the bottle, this equilibrium is violated, and it will return to the equilibrium state after closing the cap a second time later. However, in doing so, a quantity of gas has already left the bottle. Thus, the amount of carbon dioxide in the gaseous phase is kept the same (at the end of equilibrium). By shrinking the bottle, we reduce the amount of carbon dioxide that can leave the liquid (due to lack of physical space), but as the gas leaves the liquid, its pressure will gradually inflate the sides of the bottle and gradually increase its return. In fact we accomplished the opposite goal: in the initial steady state the pressure above the liquid contains air and carbon dioxide molecules. If we pumped the air in with the initial pressure, the entire pressure will (eventually) be 100 percent carbon dioxide, so we've actually allowed more gas to escape than it would have if we hadn't interfered with the process.
Therefore, if we want to reduce the escape of gas, we will have to carefully transfer the drink to a smaller bottle, or continue to keep the sides of the bottle compressed.
A final word about the second law of thermodynamics. Many think that this is some kind of decree from heaven, like many other laws. The force will always be equal to the product of the mass times the acceleration. However, the second law is not arbitrary at all, but only probabilistic. There is a real chance that all the smell from the perfume we put will concentrate in a corner of the room and not move away. There is no law that states that it will equal concentrations, just as there is no law that states that after six million throws of a die the number five will come up a million times. Only probability determines that.
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Answer to Eyal:
What are you mentioning this about?
Isn't it simpler to claim that there will be a comparison of concentrations of the gas between liquid and air?
The answer is not from the field of thermodynamics. Gases know how to maneuver through cracks because of the size of the molecules. It will not be easy for the liquid to pass through the rails of the stopper. The molecules are larger and the friction is greater. In fact, as anyone who has been cut and has a drop of blood from shaving knows, as soon as the first drop comes out, the second drop stops coming out. This is caused by the fact that the first drop has to push the first one out, but the first one is no longer under pressure because it is already outside.
The same goes for shaving. If you wipe the wound more blood will come out. Allow the drop to dry or the coagulants to clot
I wonder how right you are about this...
The gas bubble in the case of a cork that does not close hermetically will be from the same partial pressure whether the cork comes in contact with gas or liquid. Therefore, intuitively, it seems to me that the escape of the gas will be the same if there is such an escape, if the bottle is placed on its side.
Is there any kind of truth in my words? Aren't gases bubbling better through a liquid medium?
* * confused icon * *
What you say is absolutely true. Another correct point emerges from your words that if we store the bottle lying down, the gases, which naturally tend to rise inside a liquid, will remain in the middle of the bottle and will not strive to reach the cork area.
It was worth mentioning that you should place the carbonated drink bottle on its side, so that the liquid will be in contact with the cap and block the escape of gases. (For gas it is easier to bubble through the cork).
A bottle of wine is also placed on the side, but this is to keep the cork moist so that it does not dry out and cause oxygen to enter inside and oxidize the wine.
This new section is great!
Well done and thank you very much.
Ami