Molar Mass of Zinc Chromate (ZnCrO4)
Molar Mass of Zinc Chromate is commonly used in ionic-equation practice and concentration calculations for salt solutions. Molar Mass of ZnCrO₄ is 181.37 g/mol, based on 3 element types, with Zn contributing the largest share.
For fast checks, use the molar mass calculator, verify element values in the periodic table, or explore more molar mass.
Molar Mass of Zinc Chromate is:
181.37 g/mol
Molar Mass of ZnCrO₄ equals 181.37 g/mol, so 181.37 grams is one mole.
Element Breakdown Table
| Element | Count | Atomic mass | Calculation | Contribution |
|---|---|---|---|---|
| Zinc (Zn) | 1 | 65.38 | 1 x 65.38 | 65.38 g/mol |
| Chromium (Cr) | 1 | 52.00 | 1 x 52.00 | 52.00 g/mol |
| Oxygen (O) | 4 | 16.00 | 4 x 16.00 | 64.00 g/mol |
Final molar mass 65.380 + 52.000 + 64.000 | 181.37 g/mol | |||
Computing Molar Mass of Zinc Chromate Step by Step
Molar Mass of Zinc Chromate: Step-by-Step Calculation
1. Identify Element Counts
Read ZnCrO4 and list how many atoms of each element are present:
- 1 atom of Zinc (Zn)
- 1 atom of Chromium (Cr)
- 4 atoms of Oxygen (O)
2. Determine Atomic Masses
Look up each element mass from the periodic table:
- Zinc (Zn) ~= 65.380 g/mol
- Chromium (Cr) ~= 51.996 g/mol
- Oxygen (O) ~= 15.999 g/mol
3. Multiply Atomic Mass by Quantity
Multiply atom count by atomic mass for each element:
- Zinc (Zn): 1 x 65.380 = 65.380 g/mol
- Chromium (Cr): 1 x 51.996 = 52.000 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 65.380 + 1 x 51.996 + 4 x 15.999)
Molar Mass = 65.380 + 52.000 + 64.000
Molar Mass = 181.370 g/mol
Final rounded value shown on this page: 181.37 g/mol.
Visual Calculation Chart
| Element | Count | Mass | Count x mass | Contribution |
|---|---|---|---|---|
| Zinc (Zn) | 1 | 65.380 | 1 x 65.380 | = 65.380 |
| Chromium (Cr) | 1 | 51.996 | 1 x 51.996 | = 52.000 |
| Oxygen (O) | 4 | 15.999 | 4 x 15.999 | = 64.000 |
Final molar mass 65.380 + 52.000 + 64.000 | = 181.370 | |||
Easy Way to Remember
Easy way to remember Molar Mass of Zinc Chromate
- Molar Mass of Zinc Chromate: 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.
Sample Reactions
| Type | Reaction |
|---|---|
| Double displacement | AgNO₃ + NaCl → AgCl + NaNO₃ |
| Acid-salt reaction | Na₂CO₃ + ₂HCl → ₂NaCl + H₂O + CO₂ |
Do You Know?
– Zinc Chromate contains 3 element types: Zn, Cr, O.
– Zn contributes the largest share of this compound's total molar mass.
– In ZnCrO₄, O appears with the highest atom count.
– Its molar mass is 181.37 g/mol, which is used directly in gram-to-mole conversions.
– A common reaction for Zinc Chromate is double displacement (AgNO₃ + NaCl → AgCl + NaNO₃).
For more examples in the same format, browse the related formulas on molar mass guide.
Why This Compound Matters
Zinc Chromate 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 Zinc Dichromate (ZnCr2O7) and Sodium Chromate (Na2CrO4).
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 ZnCrO₄ and miscounting atoms.
- Rounding atomic masses too early before finishing all multiplication steps.
- Mixing up Zn element contribution with total molar mass.
- Reporting a value without units; final answer should be in g/mol for Zinc Chromate.
Quick Revision
Formula: ZnCrO4
Molar Mass: 181.37 g/mol
Key takeaway: count atoms accurately, multiply by atomic masses, and sum only at the end.
Formula Explanation
ZnCrO4 contains Zinc (Zn) (1), Chromium (Cr) (1), Oxygen (O) (4). Add each element contribution to get total molar mass.
FAQ
Conclusion
Molar Mass of Zinc Chromate and Molar Mass of ZnCrO₄ are now easy to revise with this structured page. You can use this method in exams, lab reports, and daily chemistry practice.