At constant temperature and capacity, inert gas is added to the gaseous equilibrium system

First of all, I would like to correct you with a misconception that the effect of pressure on the equilibrium movement of a gaseous equilibrium system is essentially the effect on the concentration of reactants, so as long as the concentration of reactants does not change, the equilibrium of the reaction will not move even if the pressure changes. At constant temperature and volume, the addition of inert gas to the gaseous equilibrium system does not change its concentration, so its chemical equilibrium is not affected.

The opposite problem is that at a constant temperature and pressure, an inert gas is added to the gaseous equilibrium system, which reduces the concentration of reactants, so that the equilibrium shifts.

The total pressure does increase, but the partial pressure of each gas does not change, nor does the concentration of each substance (in mol l), so the equilibrium does not move.

The factor that affects the balance in high school is pressure, but it is accurate to say that it is the partial pressure of various gases.

The pressure depends on the partial pressure of each component of the gas, that is, the total pressure * the amount fraction of the substance.

In fact, the ideal gas has no intermolecular interaction between the components, so the existence of other components is not ideal for the state of an ideal gas, the ideal gas components are always full of containers, the volume remains unchanged, and the partial pressure will not change under the condition that the amount and temperature of the substance remain unchanged.

pv=nrt

It can also be illustrated by analogy: under constant temperature and volume, a small amount of solid sodium chloride is added to the acetic acid solution (equilibrium system), and the pH of the solution remains unchanged after testing, which proves that the ionization equilibrium has not moved. It can be seen that at a constant temperature and capacity, as long as the concentration of particles involved in equilibrium remains unchanged, the equilibrium will not move.

The total pressure increases, but the partial pressure of each gas does not change (i.e., the concentration of each substance does not change), so the equilibrium does not move.

No. Inert gases do not affect the various equilibriums.

The chemical equilibrium of the reaction in a constant volume and constant temperature closed container added to an inert gas container does not change because the gaps between gas molecules are too large, so that gases can diffuse freely in space and exist in each other when they do not react. The volume of each gas in the space is the container volume v.

The rate of their reaction is related to the probability of collision, and the physical quantities that appear on the surface are the other partial pressures. The introduction of inert gas does not change the other partial pressures.

According to Dalton's partial pressure law, the partial pressure of the gas is equal to the pressure of the gas when it occupies the container alone, that is, the concentration of the gas at constant volume is independent of the content of the non-reactive gas of the third party.

In the current periodic table of 118 elements, there are a total of 7 inert elements, namely: helium, neon, argon, krypton, xenon, radon and gas arcane.

At room temperature and pressure, they are all colorless and odorless monoatomic gases, and it is difficult to carry out chemical reactions. Therefore, the elemental matter formed by inert elements is also called noble gas, also known as noble gas, blunt gas, and noble gas.

There are six naturally occurring noble gases, namely helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (XE) and radioactive radon (RN). On the other hand, gas (OG) is a rare gas synthesized with a very unstable nucleus and a very short half-life.

The total pressure of the gas in the container increases, but the partial pressure of the reaction gas is not affected, and the pressure in the equilibrium constant refers to the partial pressure.

Introduction: Noble gases are group 0 elements on the periodic table.

At room temperature and pressure, they are all colorless and odorless monoatomic gases, which are difficult to carry out chemical reactions. There are seven noble gases, which are helium (He), neon (Ne), argon (Ar), krypton (Krypton), xenon (Xe), radon (RN, radioactive), and gas (OG, radioactive, man-made element).

Among them, OG is a rare gas synthesized artificially, and the nucleus is very unstable, with a short half-life of only 5 milliseconds. According to the periodic law, it is estimated that OG is more reactive than radon. However, theoretical calculations suggest that it can be very lively.

However, the carbon group element Fl exhibits similar properties to noble gases.

Chemical equilibrium: a reversible reaction under certain conditions, when the positive reaction rate is equal to the reverse reaction rate, the concentration of each component in the reaction mixture remains unchanged, and the equilibrium moves: under the conditions of chemical reactions, due to the change of reaction conditions, the process of making the reversible reaction change from one equilibrium state to another equilibrium state, and the factors that affect the chemical equilibrium movement:

Concentration, pressure, and temperature.

Constant volume, the volume is constant, the addition of inert gas, means that the concentration of the reactant is not affected, the concentration = the amount of the substance volume.

Since the concentration of the components of the reaction mixture does not change, the equilibrium does not move.

For a reversible reaction with the participation of gases, the change in pressure must cause a change in the concentration of each substance, and if the concentration does not change, the equilibrium does not move.

This problem can be understood as long as it is separated according to the actual situation.

1.If the volume of the reaction vessel does not change (the volume of the fixed vessel ---i.e., the constant volume state), then if the gas charged is a gas that is independent of the reactants and products, the concentration of each reactant does not change, although the total pressure changes, and the unit volume does not change.

The effective collision probability of the internal reactants does not change, and the rate of chemical reactions.

It accelerates with the increase of the concentration of reactants, and the reaction rate does not change when the concentration of reactants does not change.

2.If the volume of the reaction vessel changes (the volume of the Tantan vessel is not fixed---i.e., the constant pressure state), with the addition of irrelevant gases, the volume of the reaction vessel increases, the concentration of each reactant decreases, and the reaction rate must decrease.

3.It is important to properly understand the principle of the effect of concentration on the reaction rate. It is also necessary to clarify which gases are irrelevant and guess the body, if they are irrelevant gases, their function is to be with noble gases.

Just treat it exactly the same.

Hope understood.

Since it is an ideal gas of a certain mass, when the temperature increases, its internal energy increases.

The ideal gas satisfies du = cv dt in any process. where CV is the constant volume heat capacity of an ideal gas. cv =n 。Ideal gas for monoatomic molecules: = 3r2

Diatomic molecule ideal gas: = 5r2

Polyatomic Molecule Ideal Gas:

For a hybrid system: , hybrid = xb, b

where n is the mass of the matter and r is the universal gas constant.

In the process of constant capacitance, CV is a fixed value. So t increases the internal energy according to the first formula.

At constant capacity, a certain amount of ideal gas, when the temperature rises,Internal energy increases. You can use:

The higher the temperature, the more intense the thermal motion of the molecule, and the increase of the kinetic energy of the molecule.

Under constant capacitance, how will the internal energy of a certain amount of ideal gas change when the temperature rises?

Summary. Hello, I'm glad to answer for you, dear, yes, a gas reduction reaction Under the addition of constant temperature and constant volume, re-enter the inert gas The pressure will change; However, for the gases involved in the reaction, because the volume of the system does not change, the concentration does not change, which does not lead to a shift in equilibrium.

A reaction in which the gas decreases with the addition of constant temperature and volume re-enters the inert gas and the pressure does not change.

Hello, I'm glad to answer for you, dear, yes, a gas reduction reaction Under the addition of constant temperature and constant volume, re-enter the inert gas The pressure will change; However, for the gases involved in the reaction, because the volume of the system does not change, the concentration does not change, which does not lead to a shift in equilibrium.

Supplementary information: constant temperature and pressure, the pressure of inert gas plus the pressure of the system = the pressure of the original system, so the pressure of the system is reduced compared with the original.

Is it true that the pressure becomes larger?

The pressure becomes greater and should not be moved.

Kiss, the pressure is smaller. At constant temperature and pressure, the pressure of the inert gas plus the pressure of the system = the pressure of the original system, so the pressure of the system is reduced compared with the original.

Because the concentrations of reactants and products do not change, the effect of pressure on equilibrium is actually affected by concentration. This situation is equivalent to increasing the volume of the container under the condition of constant temperature and constant capacity. Move in the direction of an increase in the number of gas molecules.

If inert gas is added, there are two situations: false pressurization and true decompression, the so-called false pressurization is to add inert gas or non-reactive gas with constant capacity, and the concentration of reactants remains unchanged, so the equilibrium remains unchanged but the rate is accelerated.

True decompression is the addition of inert gas or non-reactive gas to the constant pressure vessel, the volume increases, the amount of the substance remains unchanged, and the concentration of the substance decreases, so the reaction equilibrium is destroyed. In addition, the method of judging the balance of the reaction is as follows:

For the reaction, Ma(G)+NB(G) yields PC(G)+qd(g). If the temperature is constant, the constant volume: when the addition amount is equivalent to the original amount, the two equilibrium are equivalent (for the reaction with the coefficient m+n=p+q, the addition amount is proportional to the original amount, and the two balances are equivalent).

If the temperature is constant and the pressure is constant, the amount added is proportional to the original amount, and the two balances are equivalent.

The total pressure of the gas in the container increases, and the arrangement of electrons in the atoms of the noble gas element in each electron shell just reaches a stable number. It is also difficult to react chemically with other substances, so these elements are called "noble gas elements".

Among noble gas atoms with a larger atomic weight and a higher number of electrons, the outermost electrons are farther away from the nucleus and are relatively weakly bound. If you encounter other atoms that attract strong electrons, these outermost electrons are lost, resulting in a chemical reaction.

Neon, argon, krypton and xenon are obtained from air by gas liquefaction and fractionation, while helium is usually extracted from natural gas and radon is usually separated by radioactive decay of radium compounds. Rare gases are mainly used in industrial applications in lighting, welding and space exploration.

Helium is also used in deep-sea diving. If the diving depth is greater than 55 meters, the nitrogen in the compressed air cylinder used by the diver should be replaced by helium to avoid oxygen poisoning and nitrogen anesthesia. On the other hand, because hydrogen is very unstable and flammable, helium is used instead of hydrogen in today's airships and balloons.

Under constant pressure, the partial pressure of the reaction gas decreases after being filled with inert gas, and the reaction moves in the direction of increasing gas volume.

Constant temperature and pressure, the pressure can not change, then the volume of the gas reaction becomes larger. The density of each component decreases, but to varying degrees, resulting in a shift in equilibrium.