-
The total pressure of the container increases because the number of molecules of the gas increases, the volume does not change, and the pressure increases. However, it can be considered that the pressure of the original reaction system remains unchanged, which involves the problem of partial pressure, or the pressure is understood from the perspective of the concentration of the substance, the concentration of reactants and products does not change, and the pressure of the reaction system does not change.
To sum up, whether the pressure of the reaction system changes depends on the concentration. Constant temperature and volume plus rare gases, the concentration of reactant products remains unchanged, which is equivalent to the same pressure, the reaction rate remains unchanged, and the equilibrium does not move. With the addition of rare gases at constant temperature and pressure, the volume of the container increases, and the concentration of reactant products decreases, which is equivalent to reducing pressure, the reaction rate slows down, and the equilibrium moves in the direction of shrinkage.
-
Increase, calculated according to the physical formula.
Since the pressure of the gas is essentially generated by the continuous collision between a large number of gas molecules in irregular motion and the container wall, when other conditions remain unchanged, the decrease of gas volume will increase the number of collisions between the gas molecules and the container wall and increase the pressure. Filling with noble gases is equivalent to reducing volume.
-
In the case of constant capacitance, the inert gas charge has no effect on the original equilibrium and reversible reaction, because the reversible reaction looks at the partial pressure of the reactants or products, and the total gas pressure has no effect. In the case of constant pressure, the filling of inert gas is equivalent to a decrease in the partial pressure of each gaseous substance in a reversible reaction, which is equivalent to the dilution of the gas.
-
It should be said that the pressure increases, there is no doubt about it. However, as long as the noble gas does not participate in the reaction, the concentration of each reactant and the product does not change, and the equilibrium does not move.
-
Enlarged! Because the number of molecules colliding with the container wall per unit time increases!
-
Doesn't grow. I don't know where to explain it, but that's how it drops.
-
The pressure generated by the gas, from a microscopic point of view, is formed due to the irregular movement of the gas molecules and the constant impact providing a force set. A vivid example in the physics book is that a small steel ball smashed on the electronic scale will only instantly display a force value, if the small steel ball is constantly poured on the electronic scale, the electronic scale will show a relatively stable force value. The pressure of gas molecules is the continuous collision of gas molecules to produce a continuous force.
The gas mass of the closed container is unchanged, that is, the total number of gas molecules contained in it is constant, at this time, on the container wall of the same area, if there are n molecules in the original unit time to impact the force of size a, when the gas volume is reduced, the number of gas molecules in the unit volume will increase, that is, the gas density becomes larger, the same area of the container wall may have more than n molecules per unit time assuming 2n molecules, if the temperature remains unchanged, that is, the overall energy of the system is not lost, The velocity of the molecules remains unchanged, and the force generated by the collision of 2n molecules at this time will obviously be greater than a, according to the pressure p=f s, the force becomes larger, the area does not change, and the pressure seepage force becomes larger.
-
Answer]: The answer to this question is A, D.
When the volume of a certain mass of gas remains unchanged and the temperature increases, the pressure of the gas decreases, the density cavity does not change, and the average rate of Wüner touching bright molecules increases.
-
The concentration does not change.
The pressure of the gas is c = n v p = f s = nrt v.
r is a proportionality constant, which is a fixed value. t is the temperature of the system.
Obviously, p is the fixed value, then nt v is the fixed value.
Since it is a constant temperature and constant pressure condition, p and t are constant, so n v is constant.
However, it should be noted that the so-called constant temperature and pressure is the final result, not the process.
When the gas is first added, the concentration of reactants increases instantaneously, so the reaction shifts to the right.
But after equilibrium, according to the above formula, the concentration of each substance will definitely not change.
-
Regarding the reversible reaction, it is recommended that the landlord use PV (volume) = NRT (r is a constant) and the relevant basic formula for derivation. It can be concluded that C (sulfur dioxide) decreases, C (oxygen) increases, and C (sulfur trioxide) increases.
-
Because there is a certain interval between the particles that make up the substance, there is a relatively large balance between the particles that make up the gas, so it is easier to be compressed; On the other hand, the particles that make up solids and liquids have a small space, so they are more difficult to compress
Therefore, the answer is: the intermolecular interval between gases is large, while the intermolecular or slow separation between solids and liquids is small
-
It is very important to know whether the container is constant pressure or constant capacity.
Because the shift in equilibrium is ultimately due to changes in the concentration of reactants or products.
If the change in pressure does not affect the concentration, then the equilibrium does not move. (For example, there is no equation for entropy increase and entropy decrease, that is, the left and right gas coefficients are equal).
If the pressure is constant, increasing the pressure is equivalent to decreasing the volume, and the concentration of the substance increases.
According to Le Chatletre's principle, if one of the conditions affecting the equilibrium is changed, the equilibrium will move in a direction that will weaken to that extent. To increase the pressure, the equilibrium should move in the direction of reducing the pressure, that is, in the direction of reducing the volume (reducing the total amount of matter). Reduce the pressure and vice versa.
This principle is also an empirical principle, which is very important, and you will find its strength when you do it slowly.
If the volume is constant, no matter how you change the pressure in it, the concentration does not change (n=cv) and the volume does not change.
In your question, there is no relationship between pressure and gas volume, but in a container, give it the premise of constant pressure, and after changing the pressure, this premise must be satisfied, and changing the pressure is equivalent to changing the volume.
The gas itself has no volume, and the volume of this space is counted as its volume as much space as you give it.
Puzzled, he continued to ask.
-
This reaction is a reaction with the same volume, and even if the reactants or products are re-added, it is only conducive to the reaction to proceed towards or against the equilibrium. The equilibrium does not change, so the percentage content of the components does not change.
-
Under constant volume conditions, the chemical equilibrium point remains unchanged, and even if the reactants or products are re-added, it is only conducive to the reaction towards or against the equilibrium. The equilibrium does not change, so the percentage content of the components does not change.
-
Since 2Hi = I2 + H2, the amount of the total substance before and after the reaction remains unchanged, when equilibrium, other conditions remain unchanged, and then a certain amount of Hi is added, and when the equilibrium is re-reached, although the amount of Hi is increased, the amount of the reaction product is also increased to the same extent (which is equivalent to increasing the pressure to it), therefore, the filling of Hi will not affect the movement of chemical equilibrium, that is, whether the percentage content refers to the volume fraction or the quantity fraction of the substance, the percentage content of the i2 is unchanged. (For the reaction of 2Hi = I2 + H2, the percentage of each substance when the reaction reaches equilibrium is only related to temperature).
-
1) A certain amount of gas, keep the volume unchanged, then the molecular number density remains the same; When the temperature increases, the average kinetic energy of the thermal motion of the molecule increases. Therefore, the molecular impact force per unit area increases, that is, the air pressure increases;
2) If a certain amount of gas is kept at a constant temperature, the average kinetic energy of the thermal motion of the molecule remains unchanged; When the volume increases, the molecular number density decreases. Therefore, the molecular impact force per unit area decreases, that is, the air pressure decreases;
Therefore, the answer is: 1) As the temperature increases, the average kinetic energy of the molecule increases, so the pressure increases;
2) If the temperature remains unchanged, the average kinetic energy of the molecular thermal motion remains unchanged, and the volume becomes larger, the number of molecules acting on the container wall per unit area per unit time decreases, and the pressure decreases
Mother liquor: The medium commonly used in experiments can be dispensed into 10 times and 100 times the mother liquor. >>>More
After dilution of acetic acid with water, its concentration decreases, the acidity of the solution decreases, and the pH increases. After adding sodium acetate crystals, the concentration of acetate ions in the solution increases, and due to the homoionic effect, the ionization equilibrium of the original acetic acid molecules moves to the direction of the reverse reaction (inhibits ionization), the concentration of hydrogen ions decreases, and the pH also increases. >>>More
The strong alkali weak salt does not react with the alkali, because it is also alkaline, the strong acid and weak alkali salt are acidic, and it has the general nature of acid, and the strong alkali weak salt and the strong acid and weak alkali salt are strong and the nature of the salt.
Of course, there is hope, inorganic chemistry and organic chemistry are two branches of chemistry, inorganic talks about some basic and elemental knowledge, organic talks about the properties and reflection mechanism of organic compounds, etc., you can learn well, I hope you inorganic will also keep up.
This ......The one on the first floor doesn't seem to be a compulsory two, but a lot of it is in the reaction principle elective book, and the compulsory ...... doesn't have to be so difficult >>>More