Molar Mass of Acetone (C3H6O)
Molar Mass of Acetone supports organic chemistry work where composition and mass relationships are compared across carbon compounds. Molar Mass of C₃H₆O is 58.08 g/mol, based on 3 element types, with C 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 Acetone is:
58.08 g/mol
Molar Mass of C₃H₆O equals 58.08 g/mol, so 58.08 grams is one mole.
Element Breakdown Table
| Element | Count | Atomic mass | Calculation | Contribution |
|---|---|---|---|---|
| Carbon (C) | 3 | 12.01 | 3 x 12.01 | 36.03 g/mol |
| Hydrogen (H) | 6 | 1.01 | 6 x 1.01 | 6.05 g/mol |
| Oxygen (O) | 1 | 16.00 | 1 x 16.00 | 16.00 g/mol |
Final molar mass 36.030 + 6.050 + 16.000 | 58.08 g/mol | |||
Computing Molar Mass of Acetone Step by Step
Molar Mass of Acetone: Step-by-Step Calculation
1. Identify Element Counts
Read C3H6O and list how many atoms of each element are present:
- 3 atoms of Carbon (C)
- 6 atoms of Hydrogen (H)
- 1 atom of Oxygen (O)
2. Determine Atomic Masses
Look up each element mass from the periodic table:
- Carbon (C) ~= 12.011 g/mol
- Hydrogen (H) ~= 1.008 g/mol
- Oxygen (O) ~= 15.999 g/mol
3. Multiply Atomic Mass by Quantity
Multiply atom count by atomic mass for each element:
- Carbon (C): 3 x 12.011 = 36.030 g/mol
- Hydrogen (H): 6 x 1.008 = 6.050 g/mol
- Oxygen (O): 1 x 15.999 = 16.000 g/mol
4. Sum Total Molar Mass
Add all contributions to get the final molar mass in g/mol.
Molar Mass = (3 x 12.011 + 6 x 1.008 + 1 x 15.999)
Molar Mass = 36.030 + 6.050 + 16.000
Molar Mass = 58.080 g/mol
Final rounded value shown on this page: 58.08 g/mol.
Visual Calculation Chart
| Element | Count | Mass | Count x mass | Contribution |
|---|---|---|---|---|
| Carbon (C) | 3 | 12.011 | 3 x 12.011 | = 36.030 |
| Hydrogen (H) | 6 | 1.008 | 6 x 1.008 | = 6.050 |
| Oxygen (O) | 1 | 15.999 | 1 x 15.999 | = 16.000 |
Final molar mass 36.030 + 6.050 + 16.000 | = 58.080 | |||
Easy Way to Remember
Easy way to remember Molar Mass of Acetone
- Molar Mass of Acetone: 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 |
|---|---|
| Combustion | C₃H₆O + ₄O₂ → ₃CO₂ + ₃H₂O |
| Sodium reaction | ₂C₃H₆O + ₂Na → ₂C₃H₅ONa + H₂ |
Use these reactions with molar mass calculations when you need the molar mass for each species.
Do You Know?
– Acetone contains 3 element types: C, H, O.
– C contributes the largest share of this compound's total molar mass.
– In C₃H₆O, H appears with the highest atom count.
– Its molar mass is 58.08 g/mol, which is used directly in gram-to-mole conversions.
– A common reaction for Acetone is combustion (C₃H₆O + ₄O₂ → ₃CO₂ + ₃H₂O).
Why This Compound Matters
Acetone matters in organic chemistry, especially for fuel, solvent, or carbon-chain analysis.
Its formula pattern helps students practice molecular composition and yield calculation methods.
Similar calculations can be compared with Methanol (CH3OH) and Ethanol (C2H6O).
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 C₃H₆O and miscounting atoms.
- Rounding atomic masses too early before finishing all multiplication steps.
- Mixing up C element contribution with total molar mass.
- Reporting a value without units; final answer should be in g/mol for Acetone.
Quick Revision
Formula: C3H6O
Molar Mass: 58.08 g/mol
Key takeaway: count atoms accurately, multiply by atomic masses, and sum only at the end.
Formula Explanation
C3H6O contains Carbon (C) (3), Hydrogen (H) (6), Oxygen (O) (1). Add each element contribution to get total molar mass.
FAQ
Conclusion
Molar Mass of Acetone and Molar Mass of C₃H₆O are now easy to revise with this structured page. You can use this method in exams, lab reports, and daily chemistry practice.