Question

Question #551f7

Answer 1

`1.8 * 10^(23)"atoms"`

Explanation:

The idea here is that you need to use the molar mass of water to convert your sample from grams to moles, then use Avogadro's number to figure out how many molecules of water you have in the sample.

Once you know that, use water's chemical structure to calculate the number of atoms present in that many molecules of water.

So, water has a molar mass of `"18.015 g mol"^(-1)`. This tells you that one mole of water has a mass of `"18.015 g"`. You can thus use the molar mass of water as a conversion factor to calculate how many moles you have in your sample

`1.8 color(red)(cancel(color(black)("g"))) * ("1 mole H"_2"O")/(18.015color(red)(cancel(color(black)("g")))) = "0.09992 moles H"_2"O"`

Now, one mole of a molecular substance is equivalent to `6.022 * 10^(23)` molecules of said substance

`color(blue)(|bar(ul(color(white)(a/a)"1 mole" = 6.022 * 10^(23)"molecules"color(white)(a/a)|))) ->` Avogadro's number

In your case, `0.09992` moles will contain almost as many molecules as `1` mole. More specifically, you will have

`0.09992 color(red)(cancel(color(black)("moles H"_2"O"))) * (6.022 * 10^(23)"molec H"_2"O")/(1color(red)(cancel(color(black)("mole H"_2"O")))) = 6.02 * 10^(22)"molec. H"_2"O"`

As its chemical formula suggests, a molecule of water is made up of

• one oxygen atom, `1 xx "O"`
• two hydrogen atoms, `2 xx "H"`

This means that every molecule of water contains a total of `3` atoms. The number of atoms present in your sample will thus be

`6.02 * 10^(22)color(red)(cancel(color(black)("molec. H"_2"O"))) * "3 atoms"/(1color(red)(cancel(color(black)("molec. H"_2"O")))) = color(green)(|bar(ul(color(white)(a/a)color(black)(1.8 * 10^(23)"atoms")color(white)(a/a)|)))`

The answer is rounded to two sig figs.

Keep in mind that all of these atoms are locked into water molecules, meaning that there are no "free atoms" moving around in your sample.