and describe please
2007-03-07 11:29:43 · 4 answers · asked by SaxiPHNgurl3 2 in Science & Mathematics ➔ Chemistry
how do you put it in the formula , what do you do with the atomic mass?
2007-03-07 11:33:12 · update #1
6.02 x 10^23
One mole of anything will always contain Avogadro's number ( 6.02 x 10^23 ) particles.
Sample problem: (by the way - my classes have a test over this tomorrow! This better not be one of my students!)
How many atoms are present in 80.00 g Ca?
Change grams to moles: 1 mole Ca = mass Ca from table
80.00 g Ca x (1 mol Ca / 40.0 g Ca) = 2.00 mol Ca
Change moles to atoms: 1 mole Ca = 6.02 x 10^23 atoms Ca
2.00 mol Ca x ( 6.02 x 10^23 atoms Ca / 1 mol Ca ) = 1.204 x 10^24 atoms Ca.
2007-03-07 11:32:22 · answer #1 · answered by physandchemteach 7 · 0⤊ 0⤋
The same as in a mole of any element. A mole is just a number, quite a big one. A less pointless question is how heavy is a mole of Ca? You'd need the atomic weight of Ca to answer that one.
2007-03-07 19:35:37 · answer #2 · answered by Anonymous · 0⤊ 0⤋
it contain 6x10 to the power of 23 ca atom
2007-03-07 19:44:30 · answer #3 · answered by Anonymous · 0⤊ 0⤋
6.02 * 10^23 That is the same for any element it does not matter which. It is avagadro's number or something like that.
2007-03-07 19:33:55 · answer #4 · answered by Texan Pete 3 · 0⤊ 0⤋