The+Mole

=The Mole= The quantity known as the mole, also known as Avogadro's number, is equal to 6.02•10²³. You can have a mole of any substance, as long as there is a quantity of the object equal to 6.02•10²³. It is very likely that anything that can occur in a number equal to or greater than a mole that you will encounter will be atoms, molecules, or ions. For example, if you had a mole of the smallest grains of sand, its mass would be approximately 400000000000000000000 grams, or .4 zettagrams. (1 zettagram = 1.0•10²¹). If this was placed over the United States, it would create a layer approximately 3 inches thick.

Examples:
1 mol ¹²C atoms = 6.02 x 10²³ ¹²C atoms 1 mol NaCl molecules = 6.02 x 10²³ NaCl molecules 1 mol M&M's = 6.02 x 10²³ M&M's

= = =Avogadro=

Avogadro was an Italian scientist. Because of his contributions to molecular theory, the quantity of a mole is named after him.

=Molar Mass= The molar mass of an element, expressed in grams, is equal to the atomic mass of a single atom of that element. The atomic mass of carbon is equal to 12.01 amu, so the molar mass of a mole of carbon atoms is 12.01 grams. If you had the a mole of the compound C  2, its molar mass would be 24.02 (12.01•2 = 24.02).

=Sample Calculations= Calculate the following quantities:

A) mass, in grams, of 1.73 mol of CaH2 1.73 mol x 42.1 g/mol = 72.8 g CaH2

B) moles of Mg(NO3)2 in 3.25 g of this substance 3.25 g Mg(NO3)2 / 148.33 g/mol = .02191 mol Mg(NO3)2

C) number of molecules in .245 mol CH3OH .245 mol x 6.02 x 10²³ molecules = 1.45 x 10²³ CH3OH molecules

D) number of H atoms in .585 mol C4H10 .585 mol C4H10 x 6.02 x 10²³ molecules x 10 H atoms per molecule = 3.52 x 10²⁴ H atoms

This is not a mole in chemistry

Works Cited http://library.thinkquest.org/19957/atomic/molebody.html http://hypertextbook.com/facts/2003/MarinaTheodoris.shtml http://www.essex1.com/people/speer/large.html http://cal.culate.it/blog/wp-content/uploads/2009/05/a-mole.jpg