Molar Mass of Ethanol (C2H6O)
Molar Mass of Ethanol supports organic chemistry work where composition and mass relationships are compared across carbon compounds. Molar Mass of C₂H₆O is 46.07 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 Ethanol is:
46.07 g/mol
Molar Mass of C₂H₆O equals 46.07 g/mol, so 46.07 grams is one mole.
Element Breakdown Table
| Element | Count | Atomic mass | Calculation | Contribution |
|---|---|---|---|---|
| Carbon (C) | 2 | 12.01 | 2 x 12.01 | 24.02 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 24.020 + 6.050 + 16.000 | 46.07 g/mol | |||
Computing Molar Mass of Ethanol Step by Step
Molar Mass of Ethanol: Step-by-Step Calculation
1. Identify Element Counts
Read C2H6O and list how many atoms of each element are present:
- 2 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): 2 x 12.011 = 24.020 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 = (2 x 12.011 + 6 x 1.008 + 1 x 15.999)
Molar Mass = 24.020 + 6.050 + 16.000
Molar Mass = 46.070 g/mol
Final rounded value shown on this page: 46.07 g/mol.
Visual Calculation Chart
| Element | Count | Mass | Count x mass | Contribution |
|---|---|---|---|---|
| Carbon (C) | 2 | 12.011 | 2 x 12.011 | = 24.020 |
| 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 24.020 + 6.050 + 16.000 | = 46.070 | |||
Easy Way to Remember
Easy way to remember Molar Mass of Ethanol
- Molar Mass of Ethanol: 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 | C₂H₆O + ₃O₂ → ₂CO₂ + ₃H₂O |
| Sodium reaction | ₂C₂H₆O + ₂Na → ₂C₂H₅ONa + H₂ |
Do You Know?
– Ethanol contains 3 element types: C, H, O.
– C contributes the largest share of this compound's total molar mass.
– In C₂H₆O, H appears with the highest atom count.
– Its molar mass is 46.07 g/mol, which is used directly in gram-to-mole conversions.
– A common reaction for Ethanol is combustion (C₂H₆O + ₃O₂ → ₂CO₂ + ₃H₂O).
Why This Compound Matters
Ethanol 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 Propanol (C3H8O).
For broader practice beyond this compound, molar mass page keeps classroom examples one click away.
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 C₂H₆O 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 Ethanol.
Quick Revision
Formula: C2H6O
Molar Mass: 46.07 g/mol
Key takeaway: count atoms accurately, multiply by atomic masses, and sum only at the end.
Formula Explanation
C2H6O contains Carbon (C) (2), Hydrogen (H) (6), Oxygen (O) (1). Add each element contribution to get total molar mass.
FAQ
Conclusion
Molar Mass of Ethanol and Molar Mass of C₂H₆O are now easy to revise with this structured page. You can use this method in exams, lab reports, and daily chemistry practice.