What does the pressure of a certain amount of air have to do with temperature and volume?

The pressure is proportional to the temperature and inversely proportional to the volume.

It should be capitalized.

pv=nrt

r=r is the gas constant.

The relationship between the pressure, volume and temperature of the gas: the law that a gas with a certain mass obeys when the three parameters change: PV t=c (constant). P is the gas pressure, V is the gas volume, and T is the gas temperature.

PV T is the equation of state of ideal gas, also known as the ideal gas law and the universal gas law, which is an equation of state that describes the relationship between pressure, volume, quantity of matter and temperature of an ideal gas in equilibrium.

Origin: It is based on empirical laws such as Boyle-Mariott's law, Charlie's law, and Guy-Lussac's law.

At room temperature and pressure, the volume of the actual gas molecules and the interaction between the molecules are negligible, and the state parameters can basically meet the ideal gas equation of state, so aerodynamics often simplifies the actual gas to a complete gas. In low-speed aerodynamics, air can be treated as a complete gas with a constant specific heat ratio.

Summary. Within the atmospheric pressure, the higher the temperature, the greater the pressure.

Within the atmospheric pressure, the higher the temperature, the greater the pressure.

So the lower the temperature, the lower the pressure.

Why is the higher the temperature, the higher the pressure, the stronger?

Theorems discovered by physicists.

But I have seen an experiment, the experiment on the small amount of hot water poured into a plastic bottle, after a quick shake and Xiang, and then poured out the hot water, unscrewed the plastic bottle to tighten the cap and flattened, I wanted to pour hot water into the plastic bottle, the temperature inside the plastic bottle should be higher than the outside temperature, the reason for being flattened is because the pressure inside the plastic bottle is low.

This is the principle of thermal expansion and cold contraction.

So how does this experiment prove that the lower the temperature, the smaller the atmospheric pressure?

The influencing factors of atmospheric pressure are temperature, density, and altitude, while the pressure of a liquid is related to depth and density of the liquid.

This is the liquid pressure, which is not the same as the gas pressure.

I saw that this experiment was to pour out all the hot water, and after a few minutes of standing still, the bottle flattened.

I appreciate your skeptical attitude.

But I'm not a physicist or chemist myself.

Forgive me for not having that much professionalism.

I think your teacher will have a headache too.

Haha it doesn't matter.

If you're a student, hopefully you don't get into the nitty-gritty.

In the future, you will definitely be able to build materials.