marxism-digest V1 #6098

Mike Friedman mikedf at
Tue Jul 15 20:47:40 MDT 2003

Avogadro's number is the 6.02 x 1023 (ten to the twenty-third) you were 
referring to. That number of particles will give you the atomic mass of the 
substance in grams. Just to clarify.


At 09:38 PM 7/15/2003 -0400, you wrote:
>Date: Wed, 16 Jul 2003 02:05:11 +0200
>From: "Jurriaan Bendien" <bendien at>
>Subject: Avogagro's number
>Yep, Les, I am figuring out this item of terminology, thanks to the
>Internet. Sincere thanks for the idea, I must give up smoking cigarettes !
>What is a mole?
>Definition: The number of carbon atoms contained in 12.011-g carbon is 1
>mole (1 mol), which is 6.02 ´ 1023 atoms and is called the Avogagro's
>number. (C-12 is used for defining amu.)
>Or a more "general definition" as in the textbook as "The number of atoms
>(or formula units or molecules) contained in the atomic mass in g (or
>formula mass in g) of an element (or a compound)".
>Molar mass: mass in g of 1 mol of the substance
>Examples (see more on Table 4.1)
>a) water, 18 g/mol (2 mol H + 1 mol O = 2 g + 16 g), or mol/18 g
>     2 mol H atoms react with 1 mol O atoms to give 1 mol water molecules
>     (But, remember "all gases are diatomic, except noble gases." Thus,
>instead of having 2H + O ® H2O, you MUST write 2H2 + O2 ® 2H2O.)
>b) CO2, 44 g/mol (1 mol C + 2 mol O = 12 g + 16 g ´ 2), or mol/44 g
>     1 mol C reacts with 2 mol O (1 mol O2) to give 1 mol CO2;
>c) A small size protein with ~100 amino acids, ~10,000 g/mol.
>The "larger" the molecule, the more the mass is in a mole of the molecule

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