An atom of fluorine has an actual mass of 3.16x10-23grams. A mole of atoms is 6.02x1023 atoms. Using this data, calculate
the mass in grams of a mole of fluorine atoms. I have no clue how to do this any help?
2006-10-18 09:42:53 · 3 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
you just multiply 3.16x10^-23 x 6.02 x 10^23
and you get 19.0232g
the mass of one atom x the number of atoms in one mole = the mass of one mole.
The actual atomic mass of Fluorine is 18.9984032 g/mol but that is an average of all the isotopes.
2006-10-18 09:48:15 · answer #1 · answered by Anonymous · 1⤊ 0⤋
Ok.... basically 6.02 x1023 is one molecule of Flourine... that number is called avogadro's number it is constant.... so you use 3.16x10-23 and multiply by 1 mol divided by 6.02x1023 . This will give you the moles of flourine which is .5249 moles flourine.... Then you take .5249 and multiply it by the atomic mass of flourine which is 18.9984 and you get 9.97... that is the final answer
2006-10-18 16:53:12 · answer #2 · answered by Anonymous · 0⤊ 1⤋
Multiply the two numbers together!
2006-10-18 16:45:53 · answer #3 · answered by Gervald F 7 · 0⤊ 0⤋