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As far as I know, Avogrado's Number is most commonly used to find the amount of molecules/atoms in a mol of a substance. By it's formal definition, the constant itself is the number of units in one mol of any substance where the units may be electrons, ions, atoms, or molecules. If you did practice problems in Fundamentals section A or B, the constant can be used in many varying context but is most commonly used to find the amount of atoms or molecules in chemistry at least.
A good example of when to use avogadro's number can be seen in example E.1 in the textbook. The number of hydrogen atoms is given in a sample, 1.29 X 10^24 H atoms. The questions wants to know how many moles of hydrogen atoms can be stored in a hydrogen storage device. Avogadro's number comes into play when the number of hydrogen atoms is divided by the constant, because 1 mole has 6.0221 X 10^23 of something, and in this case it is atoms. The final answer is then given in moles, 2.14 mol H.
Avogadro’s number is just a quantity of something. You would typically use it to determine how many atoms are there in a compound or such like that. Since 1 mole is equal to 6.022 x10^23, you can use the number of moles you have to determine how many atoms are in that substance
Avogadro's number is used to describe a quantity of something. It is similar to the concept of a "dozen" except instead of referring to 12 of something, it refers to 6.022*10^23 of something. It is used when converting to/from moles to/from a number of molecules, formula units or atoms, among other things.
Think of 6.022x10^23 as the amount of "things" in a mole. If you have 6.022x10^23 cats you have a mole of cats. If you have 6.022x10^23 voles (a gopher-like animal) , you have a mole of voles. So, if they ask how many molecules of let's say CO2 in 4 moles, multiply 4 by 6.022x10^23, and there you go.
You want to use Avogadro's Number in order to convert mols into atoms, molecules, or formula units. If the question wants you to do this, it will specify that they are looking for such units (atoms, molecules, formula units etc).
You use Avogadro’s number when you want to covert moles into atoms. For example, when you’re given a certain number of grams, like 500 grams of NaCl, you would divide this number by the molar mass of NaCl. Then, you take the number of moles in NaCl and multiply by Avogadro’s number to get the number of atoms present.
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