Why 1 mole of different substances contains the same number of particles

We know that a substance is made up of molecules or atoms or ions, and as long as the amount of particles in this substance is about 1 mole.

Just like a case of Coke, enough for 20 cans of Coke is called a case of Coke, and the same is true for 1 mole.

It is a standard value that scientists measure, why do scientists set the number of balances as?

Because scientists take carbon as the standard, carbon is composed of multiple carbon atoms, and the relative atomic mass of carbon is 12, then the molar mass of carbon is 12 grams, and scientists have studied that 12 grams of carbon contains about one carbon atom, and then all other substances are the same law:

The relative atomic mass of the substance x = the molar mass of the substance.

is a constant.

For example: oxygen = 16 x = 16 grams.

Carbon = 14 x = 14 grams.

So 1 mole of different substances contains the same number of particles.

1mol c = 1mol h20 =

Hope it helps.

Because the stipulation is that 1 mole of matter contains the number of particles.

It is equivalent to 1g of different substances with the same weight.

Moles are defined by the number of particles, and the number of moles is the same as the number of particles. If 5 particles are defined as 1 mole, then 5 A particles are 1 mole and 5 B particles are also 1 mole. Of course, the definition of a mole is that a particle is 1 mole, just an analogy.

Mole is defined as the presence of a constant number of particles of Avogadro per mole of substance.

Because the mole unit is measured in numbers, no matter what the substance is, as long as the number is the same, then the amount of matter they are equal.

1 Mole of any substance contains the number of particles of the Avogadro constant, which is numerically approximate.

So the answer is:

The amount of matter - n, the molar mass - m, the number of particles (the number of particles) - n.

1. The amount of matter.

1) Concept: A physical quantity that indicates the number of particles contained in a substance.

2) Symbol: n

3) Unit: mol

2. Molar quality.

1) Concept: The unit bridge laughs at the quantity of the substance and the mass of the substance.

2) Symbol: M

3) Unit: g·mol-1

3. The number of particles.

The notion of particle number is a major role to be considered theoretically. In practice, mainly in chemistry, the number of particles in a given thermodynamic system needs to be determined, but in practice it is not possible to measure directly in terms of particle number. If the material is homogeneous and has a known quantity n in moles of matter, the relation of the number of particles n can be found as:

n=nna, where na is the Yafgadro constant.

1) The quantity of the substance is n, the molar mass is m, and the mass is m ==n = m m

2) The number of particles is n, and the number of the sails is n, =n=n na

Relative atomic mass refers to the ratio of the average atomic mass of any atom to 1 12 of the atomic mass of a carbon-12 atom as the standard, which is called the relative atomic mass of the atom.

Molar mass is the mass per unit mole of substance; Mole is the amount of matter in a system that contains the same number of basic units as the number of atoms of carbon-12.

When the mass of a substance is measured in grams, it is numerically equal to the relative atomic mass of the substance, in different units.

You can understand it by writing the calculation formula on a piece of paper yourself, it's simple.

It can be simply deduced by formula:

Relative molecular mass = true mass of 1 molecule (1 12 of the atomic mass of 1 C12).

1 molecule true mass 12 (1 c12 atomic mass) Eq. (1).

The molar mass of the molecule = 1 true mass of the molecule Avogadro constant Eq. (2).

Avogadro's constant = 12g (1 c12 atomic mass) Eq. (3).

Substitute (3) for (2).

The molar mass of the molecule = 1 true mass of the molecule (12g) (1 C12 atomic mass).

1 molecule true mass 12 (1 C12 atomic mass) g

Conclusion:1The relative molecular mass and the molar mass of the molecule are numerically equal, but the former is a ratio and has no unit; The latter has units of mass.

2.The molar mass is only when the mass is expressed in g, and is numerically equal to the relative molecular mass.

It is related to the regulations on the measurement of the quantity of matter and the method of calculating the relative atomic mass. The unit of quantity of a substance is mole.

Again, science stipulates that the number of microscopic particles contained in 1 mol of any particle collective is Avogadro's constant, which is equal to the number of carbon atoms contained in carbon 12.

The relative atomic mass of an atom is calculated as the ratio of the actual mass of an atom to one-twelfth of the actual mass of a carbon-12 atom. So the molar mass of the matter is numerically equal to the relative atomic mass or relative molecular mass in grams per mome.

Since the actual mass of atoms is very small, it would be very troublesome to calculate them by their actual mass, for example, the actual mass of a hydrogen atom is kilograms, and the mass of an oxygen atom is kilograms.

The mass of one carbon-12 atom is kilograms. The relative atomic mass of an element is the weighted average of the relative atomic mass of its various isotopes. The lowest number in the periodic table is the relative atomic mass.

Molar mass is measured in g mol and is numerically equal to its relative atomic mass or relative molecular mass.

The quantity of matter is the physical quantity obtained by dividing the mass of the substance by the molar mass, and numerically it is not equal to the relative atomic mass or the relative molecular mass.

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c contains an equal number of carbon atoms. 【Reviews】Early reputation.

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