Ross Hilton
05/28/2024 · Junior High School
Calculate the volume in \( \mathrm{dm}^{3} \) of 16.22 g of sulfur hexafluoride, \( S F_{6} \). ( \( A \), values: \( F=19 \), \( S=32 \) )
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To calculate the volume of sulfur hexafluoride (SF₆) in \( \mathrm{dm}^{3} \), we first need to determine the molar mass of SF₆.
The molar mass of SF₆ can be calculated as follows:
- Sulfur (S): 1 atom × 32 g/mol = 32 g/mol
- Fluorine (F): 6 atoms × 19 g/mol = 114 g/mol
Now, we can add these together to find the total molar mass of SF₆:
\[
\text{Molar mass of } SF_6 = 32 \, \text{g/mol} + 114 \, \text{g/mol} = 146 \, \text{g/mol}
\]
Next, we can calculate the number of moles of SF₆ in 16.22 g:
\[
\text{Number of moles} = \frac{\text{mass}}{\text{molar mass}} = \frac{16.22 \, \text{g}}{146 \, \text{g/mol}} \approx 0.111 \, \text{mol}
\]
At standard temperature and pressure (STP), 1 mole of any ideal gas occupies 22.4 \( \mathrm{dm}^{3} \). Therefore, we can calculate the volume of the SF₆ gas:
\[
\text{Volume} = \text{Number of moles} \times 22.4 \, \mathrm{dm}^{3}/\text{mol}
\]
Substituting the number of moles we calculated:
\[
\text{Volume} = 0.111 \, \text{mol} \times 22.4 \, \mathrm{dm}^{3}/\text{mol} \approx 2.49 \, \mathrm{dm}^{3}
\]
Thus, the volume of 16.22 g of sulfur hexafluoride (SF₆) is approximately \( 2.49 \, \mathrm{dm}^{3} \).
Quick Answer
The volume of 16.22 g of sulfur hexafluoride (SF₆) is approximately \( 2.49 \, \mathrm{dm}^{3} \).
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