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To calculate the number of moles of bromine (\( \text{Br}_2 \)) from a given mass, we can use the formula:

\[
\text{moles of bromine} = \frac{\text{mass of bromine}}{\text{molar mass of bromine}}
\]

1. **Given mass of bromine** = 878 g.

2. **Molar mass of bromine (\( \text{Br}_2 \))**:
   Since each bromine atom has an atomic mass of approximately 79.904 g/mol, the molar mass of bromine (\( \text{Br}_2 \)) is:
   \[
   79.904 \times 2 = 159.808 \, \text{g/mol}
   \]

3. **Calculation**:
   \[
   \text{moles of bromine} = \frac{878 \, \text{g}}{159.808 \, \text{g/mol}} \approx 5.493 \, \text{mol}
   \]

To match the significant figures provided in the mass (878. with three significant figures), we should round the answer to **three significant figures**:

\[
\text{moles of bromine} \approx 5.49 \, \text{mol}
\]

### Final Answer:
\[
5.49 \, \text{mol}
\]

Would you like a further breakdown of any part of this calculation?

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Here are some related questions to deepen understanding:

1. How do you determine the number of significant figures in a measurement?
2. Why is it necessary to match significant figures in scientific calculations?
3. What is the molar mass, and why is it useful in chemical calculations?
4. How would the answer change if the mass of bromine was given in milligrams instead of grams?
5. How would you calculate the moles if you had a compound instead of an element?

**Tip:** Always double-check the units in your calculations to ensure accuracy.

A chemist measures the amount of bromine liquid produced during an experiment. She finds that 878. g of bromine liquid is produced. Calculate the number of moles of bromine liquid produced. Be sure your answer has the correct number of significant digits.

Learn how to calculate the number of moles of bromine liquid given a mass of 878 g. This problem involves stoichiometry, unit conversion, and the correct use of significant figures. Suitable for high school students in Grades 10-12.

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