The pressure of the gas mixture in a closed container

The partial pressure produced by a gas in a mixture of gases is equal to the pressure produced when it occupies the entire container separately at the same temperature; The total pressure of the gas mixture is equal to the sum of the partial pressures of the gases.

This is Dalton's law of partial pressure of gas

ofpartial

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Introduction: Dalton's law of partial pressure (also known as Dalton's law) describes the properties of an ideal gas. This empirical law was observed by John Dalton in 1801.

In any mixture of gases in a container, if there is no chemical reaction between the components, each gas is evenly distributed throughout the container and produces the same pressure as if it had occupied the entire container individually [1]. That is, the pressure of a certain amount of gas in a container of a certain volume is only related to temperature. For example, at zero degrees Celsius, 1mol

Oxygen in. The pressure within the volume is.

If added to the container.

1mol of nitrogen and keep the volume of the container unchanged, then the pressure of oxygen is still.

However, the total pressure inside the container is doubled. It can be seen that the pressure generated by 1mol of nitrogen in this state is also the same.

See if there is a reaction and what kind of reaction occurs.

In a, two gases undergo a redox reaction to form elemental sulfur and water. There is not a single gas in the product that, if not exactly a complete reaction, is of course the least pressure.

The other few are not easy to react quickly if there are no special conditions in a closed container at room temperature.

So choose option A.

This kind of question looks at whether there is a reaction between gases and gases. Does the volume change after the reaction! change, which becomes smaller.

In A, H2S reacts with SO2 to form very water and S solids. So the volume is reduced.

Depending on the pressure of the gas is the maximum, then the liquid, and finally the solid, when the gas reacts to produce the liquid the pressure becomes smaller, so it is d

1.Because the density of the gas in the closed container is generally very small, and the pressure generated by the gravity of the gas itself is very small and negligible, the gas pressure is generated by the wall of the gas molecule collider, and the size is determined by the density and temperature of the gas, which has nothing to do with the gravitational force of the earth, and the pressure of the gas on the wall of the upper and lower left and right vessels is equal in size.

2.Atmospheric pressure is the pressure exerted on an object immersed in it due to the force of gravity on which the air tightly surrounds the earth. Without the gravitational pull of the Earth, there would be no atmosphere on the surface of the Earth, and thus no atmospheric pressure.

The value of the atmospheric pressure on the ground is multiplied by the surface area of the Earth, which is approximately equal to the value of the gravitational force experienced by the Earth's atmosphere. Atmospheric pressure is ultimately achieved by molecular collisions to exert pressure on the object placed in it.

Example: The following statement about gas pressure is correct (d).

a.Gas pressure is produced due to the gravitational force applied to the gas.

b.In the case of weight loss, the gas does not exert pressure on the wall.

c.The pressure of the gas on the bottom of the container is stronger than the pressure on the side walls.

d.The pressure of the gas is created due to the fact that the gas molecules are constantly colliding with the wall of the device.

Example: Which understanding of gas pressure is wrong (a).

a.The atmospheric pressure is generated by the gravity of the air on the earth's surface, so after the open bottle is sealed, the gas in the bottle is separated from the atmosphere, and its own gravity is too small, which will make the gas pressure in the bottle much less than the outside atmospheric pressure.

b.The gas pressure is created due to the constant impact of gas molecules against the wall of the device.

c.The gas pressure depends on the number of molecules per unit volume and the average kinetic energy of the molecules.

d.The average pressure per unit area of the wall when it is collided by air molecules is the pressure of the gas on the wall.

Example: A school physics interest group organizes a ** activity to estimate the number of molecules in the atmosphere around the earth. A student searched on the Internet and obtained the following physical quantity data:

The radius of the Earth r 10 m, the gravitational acceleration g of the Earth's surface, the atmospheric pressure p 10 Pa, the average molar mass of the air m kg mol, the constant of Avogadro na 10 molCan this student estimate the number of molecules in the atmosphere around the earth based on the above physical quantities? If so, please give the result; If not, please explain why.

To tell you a way to solve a problem, remember a constant. One mole of gas of any substance, in the standard state, its volume is liters. The standard state is a standard atmospheric pressure with a temperature of 0 degrees Celsius.

Now you don't tell everyone about the temperature, for the sake of simplicity, it's 0 degrees.

Process, 1, find the number of moles of carbon dioxide.

2. Find the volume of carbon dioxide in the standard state.

3. Find the pressure when the volume of carbon dioxide is compressed.

4. This pressure, plus the original pressure of the container, is the current pressure of the container.

5. Now the volume of carbon dioxide difference is cubic meters. Because it's mixed with the air. This is a mixture of imaginary qi gases that cannot be separated.

Analysis: From the Kraberon equation, it can be known: Bi Xianxun.

pv=m/m·rt

where Yun Qiao M represents the mass of the gas, M represents the molar mass, R is the constant, and T represents the Kelvin temperature (absolute temperature). Repentance.

This is the relationship between the mass and pressure of the gas!

Hope it helps!

It can be considered from a micro point of view.

Confined air assumes that no flow is just the ideal situation.

All the molecules are moving in an irregular motion.

For the inside of the container, its pressure p=fs

That is, the pressure is generated by the impact of microscopic particles.

In this case, if the gas molecules inside and outside the container are the same, the density is the same (that is, the number per unit volume), and the temperature is the same (the temperature affects the speed of the particles), then its pressure is the same.

Another way to consider it is the ideal gas equation of state pv = nrtp pressure, v volume, n moles (number of particles), r universal gas constant, t temperature.

The main satisfaction is that the other quantities are constant, and the pressure is constant.

Or an atmospheric pressure value. On the surface, the pressure of the atmosphere on the ground gas is the same as the pressure on the gas on the inner wall of the tank in space. If the canister is not strong enough, it will break, so you can imagine how forcefully the canister will do to the gas inside it while in space.

1. The pressure of a gas with a certain mass is related to: temperature and volume; The higher the temperature, the smaller the volume and the greater the pressure

2. The greater the flow velocity in the fluid, the smaller the pressure; The lower the flow velocity, the greater the pressure

So the answer is: temperature, volume; The smaller

Fun Science: Do you know what are the factors that affect pressure?

Since the molecular distance of the gas is large, the volume is only related to the intermolecular distance (temperature), not the size of the molecule (kind). Therefore, the volume of the gas mixture can only be calculated using the molar volume of the gas at that time (related to temperature and pressure). The specific algorithm is as follows:

Let v be the volume and vm be the molar volume of the gas in the current condition (the standard value is , then the amount of the substance is n=v vm