1 mole of a substance contains 6.02 x 1023 particles (molecules, atoms ...). This number (6.02 x 1023) is called the Avogadro's constant. the forumula: n = N / NA (NA is the Avogadro's number / constant; N = number of particles (molecules, atoms...) in the substance)
A mole is Avogadro's number of molecules (or, for non molecular substances, atoms or formula masses instead of molecules). This number has been determined experimentally to be about 6.022 x 1023 molecules. A mole of any pure molecular chemical substance is 6.022 x 1023 molecules of that substance.
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Imagine that you were able to count the atoms in exactly 12 grams of pure carbon-12, which has been defined to have a gram Atomic Mass of exactly 12. If you could, then it would come to 6.023*1023. If you could take 44 g, the gram molecular mass of CO2 gas, and count the number of molecules, it would be about 6.023*1023. 238 g, the approximate gram atomic mass, of uranium would have 6.023*1023 atoms.
These values of 12g, 44g and 238 g are known as one gram mole of carbon, carbon dioxide and uranium respectively.
The phrases "gram mole", "gram atomic mass", and "gram formula mass" should always be considered as single compound nouns, and any number preceding them applies to the phrase rather than to the single word "gram" with which the phrase begins.
Avogadro' Number, 6.0221367 X 1023 is the number of Molecules in 1 Gram Mole of a substance. One gram mole of Oxygen (at. no.16, at. wt. 32) has a mass of 32.00 grams and contains 6.0221367 × 1023 molecules.
The volume of one gram-mole of gas is about 22.4 l (0.791 cu. ft.) at standard temperature and pressure (0° C, 1 ATM) This is true for all gases.
Avogadro's number is the number of anything in a mole of that thing, which is 6.022 x 1023. For example, one mole of anything is 6.022 x 1023 of that thing, whether it be cars, shoes, or atoms, or molecules.
One mole contains Avogadro's number of 6.022 141 29 x 1023 particles.
A mole contains an avogadros number of molecules, formula units for chemical compounds or atoms for elements.
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The mole is the atomic weight expressed in grams.
These chemicals react in a direct proportion of one to one, measured in moles of course, not by weight. A mole of NaOH weighs more than a mole of HCl.
The name given to the number of particles in a mole is Avagadro's number/constant
Mole fraction is dimensionless. It's the amount of moles of species "A" divided by the total amount of moles in the mixture. So "mole A / mole total" equals "dimensionless". To add clarity in the use of mole fractions, one could add as "unit" mole A / mole "mixture".
It isn't. The mass of one mole of aluminum is less than the mass of one mole of copper. The number of atoms in one mole of aluminum is the same as the number of atoms in one mole of copper, which is 6.022 x 1023, also known as Avogodro's number.
A mole of any substance has the Avogadro's number of such units. As an example, a mole of hydrogen atoms is equivalent to 6.022 x 1023 atoms.
There is no relation.
The mole is the atomic weight expressed in grams.
There is no general exact relationship, because of the existence of neutrons in the nuclei of almost all elements and the lack of effect of neutrons on atomic number. An atom's gram atomic mass, however, is equal to the mass of one mole of the atoms in question.
the molecular mass of a compound and its empirical formula
Avogadro's number represents the number of units of a substance in one mole of the substance. These units may be electrons, atoms, ions, or molecules, depending on the substance.
If the Atomic Mass of an atom is x, then the mass of 1 mole of the atoms is x gram.
These chemicals react in a direct proportion of one to one, measured in moles of course, not by weight. A mole of NaOH weighs more than a mole of HCl.
No number since mole is an animal.
There are the same number of atoms in one mole of beryllium as there are in one mole of magnesium :)
Avogadro's number is the number of "elementary entities" (usually atoms or molecules) in one mole. It is 6.0221415 × 1023
No, a mole of helium gas does not have the same number of molecules as a mole of lead. This is because the number of particles in a mole is determined by Avogadro's number, which is approximately 6.022 x 10^23. Since helium is a monoatomic gas and lead is a solid with a lattice structure, the number of helium atoms in a mole is significantly larger than the number of lead atoms in a mole.