If the molar volume of any gas at the same temperature and pressure is equal, then the quantity and

First you need to correct the notion that the molar volume of any gas at the same temperature and pressure.

Equally, this statement is true; However, in the same container, different gases have the same temperature, but not different pressures. The total pressure of the container is actually the sum of the partial pressures of the different gases, and Avogadro's law should be used in this case.

The second corollary is the amount of gaseous matter in the case of isothermal isochorrance.

In a closed container of a certain volume, there are different types of gases – they have the same volume but different pressures. The sum of the partial pressures of various gases is equal to the total pressure.

So they are not gases of the same temperature and pressure, and the sum of the quantities and concentrations of their substances is equal to the total concentration.

Any gas with the same temperature and pressure is equal in molar volume, and the quantity and concentration of their substances are not equal. Because their molar amounts are not equal, such as 1 mole of hydrogen and 1 mole of carbon dioxide.

The pressure inside the container is caused by all gases, and it is a whole, and each gas has a different average molecular distance.

The volume of the container should also be taken into account, because:

The amount of matter. The concentration is related to the volume of the container.

In a closed container of a certain volume, there are various different kinds of gases, and because the gases automatically fill the whole container, they are equal in volume, regardless of whether the amount of their matter is equal or not. According to the same amount of gaseous substances of the same volume at the same temperature and pressure, the amount of various types of gaseous substances in this container is the same.

This is a contradiction, even if it is the same container, the partial pressure of various gases should be considered, and the partial pressure is a certain gas.

Gas mixtures. .

The quantity fraction of the substance.

Multiply by the total pressure.

At the same temperature and pressure, the ratio of the volume of two gases with the same vertical mass is equal to the molar mass.

inversely proportional. The relationship is established. First of all, the condition is that the number of particles contained in the substance is equal in the same volume at the same temperature and pressure, so the ratio of the volume of the substance can be converted into the amount of the substance.

ratio. We can deduce that the amount of matter of a substance is equal to the mass divided by the molar mass of the substance, i.e., n=m m, so v1 v2=n1 n2=m1 m1 m2 m2, and because the mass of the substance is equal, the ratio of the volume of the substance is equal to the inverse proportion of its molar mass.

For example, under the same conditions, 16go2 and 16gh2 have a ratio of 1 16 to the mass of their substances, and the ratio of their molar masses is 1 16, so the relationship is correct.

For gases, the particle size is negligible because the particle spacing is much larger than the particle size, and the factors that determine the slow volume of the gas are the number of particles and the particle spacing. The macroscopic factors affecting the particle spacing are temperature and pressure, when the temperature and pressure are the same, the spacing of any gas molecule is equal, so the same temperature and pressure, the volume of any gas in 1mol is equal, we call the volume of gas per unit of substance as the molar volume of gas.

In the case of being relatively small, many things can be ignored directly. For example atoms or ions in physics are electrically charged, and we study the Coulomb force. The effect of gravity is no longer considered. Because it's so small, the Coulomb force is even a billion-fold of gravity.

Although the particles of different gases are different in size, there is almost no difference in the difference between them and the distance between the particles, for example, a big fat man and a thin man on the earth stand together, and their distance from the moon is not equal, but the difference is completely unnecessary, so their distance from the moon can be regarded as equal.

It's the same concept of particle size and particle spacing.

At the same temperature and pressure, the same volume of gas contains the same amount of gas molecules (scientific fact) set the imitation volume v, the molar mass m1 m2 The amount of the substance is 1 to 2 = m1n v to m2n v = m1 to m2 to m2 to m2 The conclusion is as follows.

Density = mass comma density.

At the same temperature and pressure, the molar volume of the gas.

Same. Density surplus jujube sold = m vm

then the density is related to the molar mass.

proportional. Standard condition: density = molar mass Note that the unit rock is g l

Because Huinai shouts =m vm, vm is the molar volume of gas, and it is a constant at the same temperature and pressure.

The formula pushes the former field guide: =m mu trillion v=nm nvm=m vm

At the same temperature and under the same pressure shed nuclear fiber parts, the ratio of the density of the gas = the ratio of the relative molecular mass.

The relative molecular selling mass of hydrogen = 2

The relative molecular mass of the chain imitated gas a = 2*2 = 4a molar mass = 4g mol

According to the equation of state gas, pv=nrt

Wherein: p is reason.

Think about the pressure of the gas;

v is the volume of the ideal gas;

n is the amount of gaseous substances in an ideal gas;

r is the ideal gas constant, the universal gas constant.

t is the absolute temperature of an ideal gas.

Because n=m m, density = m v

then v=m density.

In the case of the same t p, v=m density, n=m m, is substituted into pv=nrt

The formula becomes. p(m density) = (m m)rt, and p density = rt m

So density 1 = PM1 RT, density 2 = PM2 RT, so, density 1: density 2 = m1: m2

According to the gas equation of state:

pv=nrt

p, t, r are certain, and v is proportional to n.

That is, the ratio of the volume of two gases at the same temperature and pressure is equal to the amount of matter.

is not equal to the molar mass ratio.

The equation of state for an ideal gas is PV=Nrt, where P is the pressure, V is the volume, N is the quantity of the gas's substance (unit: mol), R is a constant, and T is the temperature (thermodynamic temperature, unit: K, which is Kelvin).

1) Two gases at the same temperature and pressure, expressed by the equation, is V n equals constant, and V n=m density = constant (because v=m density, n=m m), so the ratio of the molar mass of the two gases at the same temperature and pressure is equal to the ratio of density.

2) Two gases at the same temperature and volume are expressed by the equation that p n is equal to a constant, so at the same temperature and volume, the ratio of the quantity of the substances of the two gases is equal to the ratio of pressure.