Molar Mass of Iron(II) Sulfate (FeSO4)
Molar Mass of Iron(II) Sulfate is commonly used in ionic-equation practice and concentration calculations for salt solutions. Molar Mass of FeSO₄ is 151.90 g/mol, based on 3 element types, with O contributing the largest share.
For fast checks, use the calculate molar mass, verify element values in the periodic table with molar mass, or explore more molar mass calculations.
Molar Mass of Iron(II) Sulfate is:
151.90 g/mol
Molar Mass of FeSO₄ equals 151.90 g/mol, so 151.90 grams is one mole.
Element Breakdown Table
| Element | Count | Atomic mass | Calculation | Contribution |
|---|---|---|---|---|
| Iron (Fe) | 1 | 55.84 | 1 x 55.84 | 55.84 g/mol |
| Sulfur (S) | 1 | 32.06 | 1 x 32.06 | 32.06 g/mol |
| Oxygen (O) | 4 | 16.00 | 4 x 16.00 | 64.00 g/mol |
Final molar mass 55.840 + 32.060 + 64.000 | 151.90 g/mol | |||
Computing Molar Mass of Iron(II) Sulfate Step by Step
Molar Mass of Iron(II) Sulfate: Step-by-Step Calculation
1. Identify Element Counts
Read FeSO4 and list how many atoms of each element are present:
- 1 atom of Iron (Fe)
- 1 atom of Sulfur (S)
- 4 atoms of Oxygen (O)
2. Determine Atomic Masses
Look up each element mass from the periodic table:
- Iron (Fe) ~= 55.845 g/mol
- Sulfur (S) ~= 32.060 g/mol
- Oxygen (O) ~= 15.999 g/mol
3. Multiply Atomic Mass by Quantity
Multiply atom count by atomic mass for each element:
- Iron (Fe): 1 x 55.845 = 55.840 g/mol
- Sulfur (S): 1 x 32.060 = 32.060 g/mol
- Oxygen (O): 4 x 15.999 = 64.000 g/mol
4. Sum Total Molar Mass
Add all contributions to get the final molar mass in g/mol.
Molar Mass = (1 x 55.845 + 1 x 32.060 + 4 x 15.999)
Molar Mass = 55.840 + 32.060 + 64.000
Molar Mass = 151.900 g/mol
Final rounded value shown on this page: 151.90 g/mol.
Visual Calculation Chart
| Element | Count | Mass | Count x mass | Contribution |
|---|---|---|---|---|
| Iron (Fe) | 1 | 55.845 | 1 x 55.845 | = 55.840 |
| Sulfur (S) | 1 | 32.060 | 1 x 32.060 | = 32.060 |
| Oxygen (O) | 4 | 15.999 | 4 x 15.999 | = 64.000 |
Final molar mass 55.840 + 32.060 + 64.000 | = 151.900 | |||
Easy Way to Remember
Easy way to remember Molar Mass of Iron(II) Sulfate
- Molar Mass of Iron(II) Sulfate: count atoms, multiply masses, and add totals.
- Write each element in a table so you do not miss subscripts.
- Keep 2-3 decimals during steps, then round only at the end.
Use this checklist with molar mass whenever you want a quick confidence check.
Sample Reactions
| Type | Reaction |
|---|---|
| Double displacement | AgNO₃ + NaCl → AgCl + NaNO₃ |
| Acid-salt reaction | Na₂CO₃ + ₂HCl → ₂NaCl + H₂O + CO₂ |
Do You Know?
– Iron(II) Sulfate contains 3 element types: Fe, S, O.
– O contributes the largest share of this compound's total molar mass.
– In FeSO₄, O appears with the highest atom count.
– Its molar mass is 151.90 g/mol, which is used directly in gram-to-mole conversions.
– A common reaction for Iron(II) Sulfate is double displacement (AgNO₃ + NaCl → AgCl + NaNO₃).
Why This Compound Matters
Iron(II) Sulfate appears in ionic-reaction practice and precipitation examples in school chemistry.
Its molar mass helps students move quickly between grams, moles, and concentration problems.
Similar calculations can be compared with Iron(II) Hydrogen Sulfate (Fe(HSO4)2) and Iron(II) Sulfite (FeSO3).
Where This Is Used
- Competitive exams and school chemistry tests.
- Lab work when preparing measured solutions.
- Real-world manufacturing and quality checks.
Common Mistakes When Calculating This
- Skipping subscripts in FeSO₄ and miscounting atoms.
- Rounding atomic masses too early before finishing all multiplication steps.
- Mixing up O element contribution with total molar mass.
- Reporting a value without units; final answer should be in g/mol for Iron(II) Sulfate.
Quick Revision
Formula: FeSO4
Molar Mass: 151.90 g/mol
Key takeaway: count atoms accurately, multiply by atomic masses, and sum only at the end.
Formula Explanation
FeSO4 contains Iron (Fe) (1), Sulfur (S) (1), Oxygen (O) (4). Add each element contribution to get total molar mass.
FAQ
Conclusion
Molar Mass of Iron(II) Sulfate and Molar Mass of FeSO₄ are now easy to revise with this structured page. You can use this method in exams, lab reports, and daily chemistry practice.