Whether the pressure can make the two elemental compounds combined. For example, hydrogen and oxygen

The ratio of the number of molecular bends is: 1: (1 + 75%) = 4: 7 Let a molecule contain n atoms, and the decomposition equation:

4ah3===6h2+man

then 6+m=7

m*n=4So:m=1;n=4.

That is, the formula code is late slipping: 4ah3===6h2+a4

At room temperature and pressure, the interaction between the molecules of these three gases is different:

1.Pure oxygen: The interactions between oxygen molecules are mainly intermolecular forces, including van der Waals forces and hydrogen bonding forces. Since the electronegativity between oxygen molecules is not very different, the force is small, the interaction is weak, and it is in an ideal gas state.

2.Pure hydrogen: The interaction between hydrogen molecules is also mainly intermolecular forces, in which hydrogen bonding forces play a major role. However, because the electronegativity of the hydrogen atom is very small, the hydrogen bonding force is also weak, the cavity is weak, the interaction is weak, and the hydrogen is also close to the ideal gas.

3.Pure water vapour: Water vapour is saturated, and the intermolecular interactions are the strongest of the three gases.

Because water molecules are more polar, strong hydrogen bonding forces can be formed between water molecules. In addition, the van der Waals force is also larger due to the larger water molecules. Therefore, the intermolecular positive force and interaction of water vapor are the strongest among the three gases, which are quite different from the ideal gas state.

In summary, the order of strength of the intermolecular forces of these three gases is: water vapor → hydrogen "oxygen". The intermolecular interaction of water vapor is the strongest, and the difference from the ideal gas state is the largest. The interaction between oxygen and hydrogen is weaker, and it is closer to the ideal gas.

Therefore, at room temperature and pressure, the interaction between the molecules of these three gases is different, the interaction of water vapor is the strongest of the three gases, while the interaction between oxygen and hydrogen is weaker and closer to the ideal gas.

It's not the same. At room temperature and pressure, the interaction between the molecules of these three substances is different.

Pure oxygen (O2) is a molecule formed by two oxygen atoms sharing electrons, and there are weak attractions such as van der Waals forces and hydrogen bonds between the molecules.

Pure hydrogen (H2) is a molecule formed by two hydrogen atoms sharing an electric shield without a son, and there is only van der Waals force and other attraction between them.

Pure water vapor is a gaseous state formed by water molecules (filial H2O) in the saturated state of caution, and there are strong interactions such as hydrogen bonds between their molecules, which are stronger than the interactions between oxygen and hydrogen.

Therefore, the interactions between the molecules of these three substances are different.

At room temperature and pressure (about 20 degrees Celsius, 1 atmosphere), the molecular interactions between 1 cubic meter of pure oxygen, pure hydrogen, and pure water vapor (saturated state) are different. Here are some of the differences between them:

The interaction between the oxygen (O2) and hydrogen (H2) molecules is mainly the van der Waals force, which is the force of attraction between the molecules. Van der Waals forces are divided into three categories: dispersion forces (also known as London forces), fundamental dipole-induced dipole forces (Debye force), and dipole-dipole forces (Krak force).

In the case of oxygen and hydrogen, the main contribution comes from the dispersion force as they are both non-polar molecules. However, the van der Waals force of the oxygen molecule will be slightly stronger because it has a larger electron cloud than the hydrogen molecule.

The interaction between water vapor (H2O) molecules is mainly hydrogen bonding. Water molecules are polar molecules in which oxygen atoms are negatively charged and hydrogen atoms are positively charged. This charge distribution causes hydrogen bonds to form between water molecules, which is a strong intermolecular force.

In contrast, hydrogen bonding is much stronger than van der Waals forces.

Therefore, among the three gases, pure water vapor has the strongest intermolecular interaction, followed by oxygen, and hydrogen has the most violent and weak intermolecular interaction. The difference in the strength of the interaction affects some of the physical and chemical properties of the gas, such as the viscosity, diffusion rate, and solubility of the gas.

I guess it's different.

It depends on the characteristics of the reaction, the characteristics of the container.

N2(g) +3H2(G) =2NH3(G) is a gas before and after, so the total mass of the gas is conserved and unchanged.

If the constant capacity container, that is, the volume of the container is unchanged, then the density = m v, unchanged.

The relative molecular mass = m n, the mass does not change, n decreases, so the average relative molecular weight increases.

If a constant pressure vessel, i.e. a reaction takes place, the volume of the vessel will gradually decrease, and the density will gradually increase.

The relative molecular weight still increases.

Co(g) +H2O(g) = CO2(g) +H2(g) are all gases before and after, and the mass remains unchanged.

The volume of the gas also does not change.

Therefore, whether it is a constant capacity container or a constant pressure container, the density before and after remains unchanged, and the relative molecular mass remains unchanged.

C(s) +H2O(G) = Co(G) +H2(G) is preceded by solids, so the mass of the gas increases.

The volume of the front and rear gases is also increasing.

If the volume of the container is constant, the mass of the gas increases, and the volume does not change, and the density increases.

If the mass of the gas increases and the volume of the gas increases, it is difficult to judge the density.

The relative molecular mass = m n, the mass increases, n also increases, so it depends on the situation of the initial addition of the substance to calculate and judge.

The volume of gas before and after the reaction remains the same, and no solid liquid participates in the reaction and is generated, all unchanged! Tell me about the equation! I'll give you the answer!

Oxygen and liquid oxygen can support combustion, water electrolysis into hydrogen and oxygen - the molecule is the smallest particle that maintains the chemical properties of the substance, in the chemical reaction the molecule can be divided into 100ml of alcohol and 100ml of water mixed in a less than 200ml - there is an interval between the molecules, the mass and volume of the molecule are very small.

"Mix in the same volume"At the same temperature and pressure, the ratio of the quantities of different gaseous substances is equal to the volume ratio, that is, these four gases are mixed with the same amount of substances, and the same number x can be set.

2a = 2b + c + 3d (the products are all gases), with 2mola decomposition to generate 6mol gas, the average phase of the mixed gas absolute spring grinding posture mass: 2 m(a) 6, the relative density of hydrogen is: 2 m(a) 6 2 m(a) 6