Question
The chemical formula for zinc nitrate is: \[ \mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2} \] Calculate the molar mass of zinc nitrate. Round your answer to 1 decimal place.
Ask by Ward Huang. in the United States
Feb 03,2025
Real Tutor Solution
Tutor-Verified Answer
Answer
The molar mass of zinc nitrate is **189.4 g/mol**.
Solution
To calculate the molar mass of zinc nitrate, \(\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}\), follow these steps:
1. **Identify the number of each atom in the formula:**
- **Zn (Zinc):** 1 atom
- **N (Nitrogen):** 2 atoms (since there are two \(\mathrm{NO}_{3}\) groups)
- **O (Oxygen):** 6 atoms (each \(\mathrm{NO}_{3}\) group has 3 oxygens, and there are two groups)
2. **Use the atomic masses (in g/mol):**
- **Zn:** 65.38 g/mol
- **N:** 14.01 g/mol
- **O:** 16.00 g/mol
3. **Calculate the total molar mass:**
\[
\text{Molar Mass} = (1 \times 65.38) + (2 \times 14.01) + (6 \times 16.00)
\]
\[
\text{Molar Mass} = 65.38 + 28.02 + 96.00
\]
\[
\text{Molar Mass} = 189.40 \text{ g/mol}
\]
4. **Round to one decimal place:**
\[
\text{Molar Mass} \approx 189.4 \text{ g/mol}
\]
**Final Answer:**
The molar mass of zinc nitrate is **189.4 g/mol**.
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Simplify this solution Extra Insights
To find the molar mass of zinc nitrate \(\mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2}\), we need to sum the molar masses of each component: - Zinc (Zn): 65.38 g/mol - Nitrogen (N): 14.01 g/mol (there are 2 in the formula) - Oxygen (O): 16.00 g/mol (there are 6 in the formula because of 3 oxygens per nitrate and 2 nitrates) Calculating: 1. Zinc: \( 1 \times 65.38 = 65.38 \, \text{g/mol} \) 2. Nitrogen: \( 2 \times 14.01 = 28.02 \, \text{g/mol} \) 3. Oxygen: \( 6 \times 16.00 = 96.00 \, \text{g/mol} \) Now, add them together: \[ 65.38 + 28.02 + 96.00 = 189.40 \, \text{g/mol} \] Therefore, the molar mass of zinc nitrate, rounded to one decimal place, is \( 189.4 \, \text{g/mol} \).
