Question

Show ALL your work! Your answer should have 3 significant figures and include units.

Moles Atoms Practice W.S. ​

Answer 1

1. 4.00 moles of
`Cu(CN)_2` corresponds to
`\(2.409 * 10^(24)\)` atoms or molecules.

2. 70.9 moles of Au corresponds to
`\(4.266 * 10^(25)\)` atoms or molecules.

3.
`\(1.19\)` moles of
`FeCl_3` corresponds to
`\(7.1558 * 10^(23)\)` atoms or molecules.

To find the number of atoms or molecules from the number of moles, you can use Avogadro's number, which is approximately
`\(6.022 * 10^(23)\)` particles per mole. The formula to convert moles to atoms or molecules is:

`\[ \text{Number of particles} = \text{Number of moles} * \text{Avogadro's number} \]`

1. For
`\(4.00\)` moles of
`\(Cu(CN)_2\)`:

`\[ \text{Number of atoms or molecules} = 4.00 \, \text{moles} * 6.022 * 10^(23) \, \text{particles/mole} \]`

`\[ \text{Number of atoms or molecules} = 2.409 * 10^(24) \, \text{atoms or molecules} \]`

2. For
`\(70.9\)` moles of
`\(Au\)`:

`\[ \text{Number of atoms or molecules} = 70.9 \, \text{moles} * 6.022 * 10^(23) \, \text{particles/mole} \]`

`\[ \text{Number of atoms or molecules} = 4.266 * 10^(25) \, \text{atoms or molecules} \]`

3. For
`\(1.19\)` moles of
`\(FeCl_3\)`:

`\[ \text{Number of atoms or molecules} = 1.19 \, \text{moles} * 6.022 * 10^(23) \, \text{particles/mole} \]`

`\[ \text{Number of atoms or molecules} = 7.1558 * 10^(23) \, \text{atoms or molecules} \]`.