Although he no longer remembers when or where he learned it, among the thousands of truths he has mastered, Mr. Seamus clearly remembers one law - Henry's Law. Pen | fun | pavilion www. ｂｉｑｕｇｅ。 ｉｎｆｏ

The so-called Henry's law refers to an empirical law summarized by the British chemist W. Henry in 1803 when he studied the solubility of gases in liquids.

Specifically, it reads: "At a certain temperature and pressure, the solubility of a gas in a liquid is directly proportional to the equilibrium pressure of the gas".

This law applies if the equilibrium partial pressure of the gas is not large, and the gas does not interact with the solvent in solution (or reacts somewhat, but is rarely ionized).

In addition to this, Henry's law is closely related to a natural phenomenon, which is the boiling point.

Taking the most common liquid water as an example, it is generally known that the boiling point of water is 100 degrees Celsius. But those who climb the mountain also know that when cooking food on the top of a mountain, the boiling point of water is lower than when it is at sea level.

This is because the air pressure at the top of the mountain is much lower than at sea level, which means that the air at the top of the mountain will feel thinner. There, water is able to boil at temperatures below 100°C.

Similarly, the lower the air pressure, the less likely it is for liquid molecules to come together, so it is easier for them to turn into gases. So, if you want to boil cold water, just lower the air pressure around you, and that's "Henry's Law".

Because in the case of liquids, although the molecules move more freely, they attract each other and form a set. When the pressure of the vapor is strong enough to overcome this attraction, bubbles are formed and the liquid begins to boil.

One might ask, what is the use of knowing such a law?

If you're a mountaineer, he'll tell you that if you don't know Henry's Law and don't have a pressure cooker, you'll only be able to eat raw food after cooking on the mountain.

But Mr. Seamus will tell you that he can use Henry's Law to create an ingenious explosion.

Yes, a happy explosion.

There is no useless scientific knowledge in this world, only mediocre people who will not turn it into an explosion.

Under normal circumstances, when a certain liquid is heated, the heat penetrates gradually, and there are many imperfections on the surface of the container.

When the liquid reaches its boiling temperature, it transforms from liquid form to gaseous form.

Since the heat is conducted through the container and the surface of the container is uneven, the liquid will gradually form small bubbles on the rough surface of the container.

The bubbles will gradually expand, a process called "gathering and expanding" - what we commonly call boiling.

As the liquid boils, these bubbles quickly grow larger and larger, eventually turning into gases and forming an "explosion".

However, an explosion of this magnitude is only a minimal chemical phenomenon, and the only power is to destroy a thin film of water.

But according to Henry's Law, it can be learned that the process of "accumulation and gradual expansion" of small bubbles and vapors produced by boiling liquids depends on air pressure and temperature.

So after making full use of Henry's Law and repeated experiments to control the changes in air pressure and gas types, Mr. Seamus discovered two important facts:

When the air pressure is low to a certain level, water can boil without heating.

When water dissolves more gas at room temperature, it will produce more gas when it boils.

So imagine if in a closed environment, if the water itself is in a critical state that is about to boil but is not boiling, what would happen if the surrounding air pressure was rapidly reduced?

Is the answer boiling?

Yes, that's right.

However, there doesn't seem to be much connection to that powerful explosion.

Don't be in a hurry.

What if Mr. Seamus replaced a condition in his experiment?

Instead of water molecules with low solubility at room temperature, choose a dieether-like liquid that can dissolve a large amount of gas at room temperature and has a boiling point as low as 32 to 34 degrees Celsius?

First, Mr. Seamus found a plastic container that was strong enough to serve as the inner container, and added a certain amount of high-temperature dieether to it.

Then a large amount of non-peroxide gas is added to the boiling dieether liquid, so that the boiling point of the diether that was originally in the boiling state rises, and finally it is not boiling.

Then the previous container is sealed and put into a larger outer container, and the outer container is filled with more gas, noting that this gas must be a gas with good temperature conductivity.

During the inflating process, the container and gas are cooled and maintained by means of a device to reach 20 to 25 degrees Celsius.

Then continue to inflate until the air pressure inside the outer container is in equilibrium with the air pressure in the inner container and is well above the normal atmospheric pressure.

When these conditions are met, the outer container is sealed.

In this way, Mr. Seamus made up of two containers, one large and one small, and filled with temperature-conducting gases in between.

After that, Mr. Seamus then warmed the temperature of the container with his own body temperature and maintained it at about 32 degrees Celsius.

At this time, because the air pressure inside the two containers is much higher than the normal atmospheric pressure, the dieether-like substance does not boil although it has reached the boiling point at normal air pressure.

Because the boiling point of the liquid inside the device is much higher than the normal 32 degrees Celsius.

Then, if necessary, open a large enough gap in the outer container, at which point the imbalance of air pressure inside and outside the outer container will cause the gas from the middle layer to flow quickly into the air.

As a result, the boiling point of the diether-like liquid in the inner container will be reduced to 32 degrees Celsius in an instant, causing the die-like liquid to boil again.

Remember what happens when you boil?

That's right, bubbles!

Don't forget that in the previous treatment of Simothy, the dieether-like liquid at this time had dissolved more non-perperoxide gases than normal.

This results in the release of more and greater amounts of gas than normal while the liquid boils, further increasing the pressure of the inner vessel.

And the whole process will be completed in a very short time, and at that time, all Seamus will get is an explosion of scientific truth and wisdom.

By the way, because the boiling point of a dieether-like liquid is the temperature of the human body, a person who is attacked by the liquid will not be subjected to secondary damage such as burning after an explosion. Moreover, the die-like ether is different from the die-ether and is not toxic, but at the same time, it has a special fragrance like the die-ether.

As for what kind of scent it is, please ask the chemistry teacher, and of course it is okay to ask the health and physical education teacher, if the school has this course.