Question
The chemical formula for lithium fluoride is LiF . A chemist determined by measurements that 0.030 moles of lithium fluoride participate in a chemical reaction. Calculate the mass of lithium fluoride that participates. Be sure your answer has the correct number of significant digits.
Ask by Valdez Macdonald. in the United States
Feb 03,2025
Real Tutor Solution
Tutor-Verified Answer
Answer
0.78 g of lithium fluoride participates in the reaction.
Solution
To calculate the mass of lithium fluoride (LiF) that participates in the reaction, follow these steps:
1. **Determine the Molar Mass of LiF:**
- **Lithium (Li):** ≈ 6.94 g/mol
- **Fluorine (F):** ≈ 19.00 g/mol
- **Total Molar Mass of LiF:**
\( 6.94 \, \text{g/mol} + 19.00 \, \text{g/mol} = 25.94 \, \text{g/mol} \)
2. **Calculate the Mass Using the Number of Moles:**
\[
\text{Mass} = \text{Moles} \times \text{Molar Mass} = 0.030 \, \text{mol} \times 25.94 \, \text{g/mol} = 0.7782 \, \text{g}
\]
3. **Apply Significant Figures:**
- The number of moles (0.030) has **two significant digits**.
- Therefore, the mass should also be reported with **two significant digits**.
- Rounded to two significant figures: **0.78 g**
**Answer:**
0.78 g of lithium fluoride participates in the reaction.
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Simplify this solution Mind Expander
To find the mass of lithium fluoride (LiF) that participates in the reaction, we first need to determine its molar mass. Lithium (Li) has a molar mass of approximately 6.94 g/mol, and fluorine (F) has a molar mass of about 19.00 g/mol. Therefore, the molar mass of LiF is 6.94 g/mol + 19.00 g/mol = 25.94 g/mol. Next, we can use the following formula to find the mass: Mass = moles × molar mass Mass = 0.030 moles × 25.94 g/mol = 0.7772 g. Considering significant figures based on the initial number of moles (0.030 has two significant figures), the mass of lithium fluoride that participates in the reaction is 0.78 g.
