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Formerly known as Moore, gram atom. The unit of quantity of matter, the symbol is mole. A mole of any substance contains
The number of structural particles is equal to the number of carbon atoms contained in 0.0 12kg 12C (carbon), i.e.
6.02 1367x 10 23。 Structural particles of daughter. Can be molecules, atoms, ions, electrons or other particles,
And specific combinations of these particles. Sometimes, the mass of one mole of a substance is called the molar mass of the substance.
Represented by the symbol μ, such as μ of hydrogen H2 = 202x10-3kg. For a substance with a mass f of m, the ratio of m to μ is called
The quantity of a substance (also called the number of moles) = mμ. For example, m = 404x10-3kg of hydrogen H2 = 2. one
The volume Vm occupied by molar substances is called molar volume. The molar volume of gas depends on temperature and pressure.
In the quasi-state, the VM of the ideal gas is 224 14 10L. Fmol- 1. Molar volume and temperature of solid and liquid substances.
There is little relationship between temperature and pressure.
Mole is the unit to express the amount of matter, and each mole of matter contains Avon Gadereau constant particles.
According to the accurate determination of scientific experiments, we know the carbon atoms contained in carbon with a relative atomic mass of 12g.
The figure is about 6.02× 10 23.
Scientifically, the collective containing 23 particles of 6.02×10 is regarded as a unit, called mole, which is a table.
The unit (symbol n) representing the quantity of a substance is simply called Mo, and the unit symbol is mol.
The carbon atom of 1mol contains 6.02× 10 23 carbon atoms, and its mass is 12g.
The sulfur atom of 1mol contains 6.02× 10 23 sulfur atoms, and its mass is 32g.
Similarly, the mass of any substance in 1 is in grams, which is numerically equal to the relative origin of atoms.
Sub-mass (formula quantity).
The molecular formula of water is 18, the mass of 1mol is 18g, and it contains 6.02× 10 23 water molecules.
Generally, the mass of 1mol substance is called the molar mass of the substance (symbol m), and the molar mass is
The unit is gram/mole, which is pronounced as "gram per mole" (the symbol is "gram per mole"). For example, the molar mass of water is
18g/mol, written as m (H2O) = 18g/mol.
How are the mass (m), quantity (n) and [1] molar mass (m) related to each other?
What kind of relationship? Existing: n=m/M
Chemical equations can express the ratio of quantity and mass of substances between reactants and products. example
For example:
The ratio of coefficients is 2∶ 1∶2.
The ratio of particle number is 2∶ 1∶2.
The ratio of substances is 2∶ 1∶2.
The mass ratio is 4∶32∶36.
It can be seen from the above analysis that the ratio of the coefficients of substances in chemical equations is the amount of substances between them.
The proportion of. Using this principle, we can calculate the amount of each substance according to the chemical equation.
The unit of quantity of matter, with the symbol of mole, is one of the seven basic units of the international system of units. Moore is a series.
The number of elementary particles in the system is equal to the number of atoms in 12g 12C. Use moles
When elementary particles should be specified, they can be atoms, molecules, ions and other particles, or they are specific to these particles.
Combination.
C (carbon) 12= 12, which is the international standard (formula) of relative atomic mass. It is known that 12g 12C contains
6.022 1367× 10 23 carbon atoms. This number is called Avon Gadereau number, so it can also be said that Avon is included.
The number of elementary particles in Garderot is 1mol. For example, 1mol oxygen molecule contains 6.022 1367×
10 23 oxygen molecules. Its mass is 3 1.9988g 1mol, and the hydrogen ions contain 6.0221367×10.23 hydrogen ions.
Son, its mass is1.00794g.
Moore in June of 197 1, 10, the 14 international metrology congress with 4 1 countries participated decided to increase it.
The seventh basic unit of the International System of Units (SI). Moles are used to calculate the number of particles and the mass of matter.
Quantity, gas volume, solution concentration, heat change during the reaction, etc. Moore comes from Latin.
Moles, originally meant to be big and piled up.
197 1 The definition of Moore in the 14th International Metrology Conference has the following two paragraphs: "Mole is one.
The amount of substances in the system and the number of basic units contained in the system are in phase with the atomic number of 0.0 12kg carbon-12.
Wait a minute. ""When using moles, you should specify the basic unit, which can be atoms, molecules, ions and electrons.
Or a specific combination of these particles. "The last two paragraphs should be considered as a whole.
The number of carbon atoms in 0.0 12kg carbon-12 nuclide is Avon Garderot constant (NA).
The approximate value is Na = 6.02× 10 23. Moles are different from ordinary units. It has two characteristics: ①.
It measures microscopic basic units, such as molecules and ions, and cannot be used to measure macroscopic substances. ②
It uses Avon Gadereau number as the unit of measurement, which is a batch, not a number, to measure particles such as molecules and atoms.
The number of. It can also be used to measure specific combinations of microscopic particles, for example, substances that measure sulfuric acid by mole.
The amount, namely 1mol sulfuric acid contains 6.02× 1023 sulfuric acid molecules. Molar is the most widely used meter in chemistry.
Bit, such as for the calculation of chemical reaction equation, calculation in solution, preparation of solution and its dilution.
The calculation of chemical equilibrium, molar volume of gas and thermochemistry can not be separated from this basic unit.
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