Question

Question #fd577

Answer 1

`1.7 * 10^(-24)` `"g"`

Explanation:

All you have to do here is to use Avogadro's constant and the mass of `1` mole of carbon as a conversion factor to go from the mass of `1` mole of atoms of carbon to the mass of `1` atom of carbon.

So, you should know that, by definition, a mole of carbon must contain `6.022 * 10^(23)` atoms of carbon. In other words, if you don't have `6.022 * 10^(23)` atoms of carbon in your sample, then you don't have `1` mole of carbon.

`"1 mole C" = 6.022 * 10^(23)` `"atoms of C " ->` Avogadro's constant

Now, you know that the mass of `1` mole of carbon, i.e. the molar mass of carbon, is equal to `"12 g"`.

This is equivalent to saying that the mass of `6.022 * 10^(23)` atoms of carbon is equal to `"12 g"`.

Therefore, you can say that the mass of a single atom of carbon will be equal to

`1 color(red)(cancel(color(black)("atom C"))) * "12 g"/(6.022 * 10^(23)color(red)(cancel(color(black)("atom C")))) = color(darkgreen)(ul(color(black)(1.7 * 10^(-24)color(white)(.)"g")))`

The answer is rounded to two sig figs.