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##4.63*10^-20## gram

You can get to the answer in two steps:

- calculate: 500 atoms = ##color(red)x## mol ?

using Avogadro’s constant. - calculate: ##color(red)x## mol = ##color(red)?## grams,

using the atomic mass of Iron.

**Step 1**

Avogadro’s constant says that ##1## mole of any atom contains ##6.022*10^23## atoms. In this case you have ##500## atoms:

##(500 color(red)cancel(color(black)(“atoms”)))/ (6.022*10^23 color(red)cancel(color(black)(“atoms”))/”mol”## = ##8.30*10^-22 mol##

**Step 2**

The atomic mass of iron (Fe) will give you the weight of one mole of this molecule: ##1## mol = ##55.845## gram:

##55.845 g/(color(red)cancel color(black)”mol”) * 8.30*10^-22 color(red)cancel color(black)”mol”## = ##4.63*10^-20 g##

So the 500 iron atoms weigh ##color(red)(4.63*10^-20) color(red)”grams”##.

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