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This worksheet seems to ask for calculating the molar mass of ammonium sulfate, \((\text{NH}_4)_2\text{SO}_4\), by breaking down the total mass of each element in the compound. Let’s go through each step needed to fill in the table:

1. **Identify each element in the compound**:
   - Nitrogen (N)
   - Hydrogen (H)
   - Sulfur (S)
   - Oxygen (O)

2. **Determine the number of atoms of each element**:
   - There are 2 ammonium ions \((\text{NH}_4)^+\), so:
     - Nitrogen (N): \(2 \times 1 = 2\) atoms
     - Hydrogen (H): \(2 \times 4 = 8\) atoms
   - Sulfur (S): 1 atom
   - Oxygen (O): 4 atoms

3. **Find the atomic mass of each element** (using average values in atomic mass units, \( \text{g/mol} \)):
   - Nitrogen (N): 14.01 g/mol
   - Hydrogen (H): 1.008 g/mol
   - Sulfur (S): 32.07 g/mol
   - Oxygen (O): 16.00 g/mol

4. **Calculate the total mass for each element**:
   - **Nitrogen**: \(2 \times 14.01 = 28.02\) g
   - **Hydrogen**: \(8 \times 1.008 = 8.064\) g
   - **Sulfur**: \(1 \times 32.07 = 32.07\) g
   - **Oxygen**: \(4 \times 16.00 = 64.00\) g

5. **Total Molar Mass of \((\text{NH}_4)_2\text{SO}_4\)**:
   - Add up the masses: \(28.02 + 8.064 + 32.07 + 64.00 = 132.154\) g/mol

### Table (Completed):

| Element | Calculations                   | Total Element Mass (g) |
|---------|--------------------------------|-------------------------|
| N       | \(2 \times 14.01\)             | 28.02                   |
| H       | \(8 \times 1.008\)             | 8.064                   |
| S       | \(1 \times 32.07\)             | 32.07                   |
| O       | \(4 \times 16.00\)             | 64.00                   |
| **Total Molar Mass** |                    | **132.154**             |

Would you like more details on the calculations or further explanation?

### Related Questions

1. What is the significance of molar mass in chemistry?
2. How do you determine the molar mass for a compound with more complex ions?
3. Why is the molar mass important in stoichiometric calculations?
4. How do changes in atomic masses affect calculations in chemical formulas?
5. What are some common applications of molar mass in laboratory settings?

### Tip
When calculating molar masses, remember to multiply each element’s atomic mass by its quantity in the formula to ensure accuracy.

Calculate the molar mass of ammonium sulfate, \((\text{NH}_4)_2\text{SO}_4\), by breaking down the total mass of each element in the compound.

Learn to calculate the molar mass of ammonium sulfate ((NH4)2SO4) by determining the total mass of each element. This guide covers key chemistry concepts, including stoichiometry and molar mass calculations, and is suitable for high school chemistry students.

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