You discover that the head of a match 1.6 grams of Sulfur, S. How many atoms of S does a match contai?

To calculate how many sulfur (S) atoms are in a match containing 1.6 grams of sulfur, we'll follow these steps:

1. **Molar mass of sulfur**: Sulfur (S) has an atomic mass of about 32.06 grams per mole.

2. **Use of Avogadro's number**: One mole of any element contains Avogadro's number of atoms, which is approximately \(6.022 \times 10^{23}\) atoms.

### Calculation:

\[
\text{Number of moles of S} = \frac{\text{Mass of S}}{\text{Molar mass of S}} = \frac{1.6 \, \text{g}}{32.06 \, \text{g/mol}} = 0.0499 \, \text{mol}
\]

Now, multiply by Avogadro's number to find the number of atoms:

\[
\text{Number of atoms} = 0.0499 \, \text{mol} \times 6.022 \times 10^{23} \, \text{atoms/mol}
\]

Let's calculate that.

\[
\text{Number of atoms} \approx 3.00 \times 10^{22} \, \text{atoms}
\]

Thus, a match containing 1.6 grams of sulfur has approximately **\(3.00 \times 10^{22}\)** sulfur atoms.

Would you like more details on any step?

### Relative questions:
1. What is a mole in chemistry?
2. How is Avogadro's number used in chemical calculations?
3. What is the significance of molar mass in chemical reactions?
4. How does the atomic mass of sulfur compare to other elements?
5. How would you calculate the number of molecules in a compound?

### Tip:
Always ensure the units are consistent (grams, moles, etc.) when doing chemical calculations to avoid mistakes!

You discover that the head of a match contains 1.6 grams of Sulfur, S. How many atoms of S does a match contain?

Learn how to calculate the number of sulfur atoms in 1.6 grams of sulfur using the mole concept and Avogadro's number. This problem explains key chemistry concepts such as molar mass and Avogadro's law. Suitable for high school students (Grades 9-12).

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