Molar Mass of Chloromethane (C1H3Cl)
Molar Mass of Chloromethane is helpful for yield calculations and formula checks in carbon-chain reaction questions. Molar Mass of C₁H₃Cl is 50.48 g/mol, based on 3 element types, with Cl 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 Chloromethane is:
50.48 g/mol
Molar Mass of C₁H₃Cl equals 50.48 g/mol, so 50.48 grams is one mole.
Element Breakdown Table
| Element | Count | Atomic mass | Calculation | Contribution |
|---|---|---|---|---|
| Carbon (C) | 1 | 12.01 | 1 x 12.01 | 12.01 g/mol |
| Hydrogen (H) | 3 | 1.01 | 3 x 1.01 | 3.02 g/mol |
| Chlorine (Cl) | 1 | 35.45 | 1 x 35.45 | 35.45 g/mol |
Final molar mass 12.010 + 3.020 + 35.450 | 50.48 g/mol | |||
Computing Molar Mass of Chloromethane Step by Step
Molar Mass of Chloromethane: Step-by-Step Calculation
1. Identify Element Counts
Read C1H3Cl and list how many atoms of each element are present:
- 1 atom of Carbon (C)
- 3 atoms of Hydrogen (H)
- 1 atom of Chlorine (Cl)
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
- Chlorine (Cl) ~= 35.450 g/mol
3. Multiply Atomic Mass by Quantity
Multiply atom count by atomic mass for each element:
- Carbon (C): 1 x 12.011 = 12.010 g/mol
- Hydrogen (H): 3 x 1.008 = 3.020 g/mol
- Chlorine (Cl): 1 x 35.450 = 35.450 g/mol
4. Sum Total Molar Mass
Add all contributions to get the final molar mass in g/mol.
Molar Mass = (1 x 12.011 + 3 x 1.008 + 1 x 35.450)
Molar Mass = 12.010 + 3.020 + 35.450
Molar Mass = 50.480 g/mol
Final rounded value shown on this page: 50.48 g/mol.
Visual Calculation Chart
| Element | Count | Mass | Count x mass | Contribution |
|---|---|---|---|---|
| Carbon (C) | 1 | 12.011 | 1 x 12.011 | = 12.010 |
| Hydrogen (H) | 3 | 1.008 | 3 x 1.008 | = 3.020 |
| Chlorine (Cl) | 1 | 35.450 | 1 x 35.450 | = 35.450 |
Final molar mass 12.010 + 3.020 + 35.450 | = 50.480 | |||
Easy Way to Remember
Easy way to remember Molar Mass of Chloromethane
- Molar Mass of Chloromethane: 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 |
|---|---|
| Synthesis | ₂H₂ + O₂ → ₂H₂O |
| Combustion | CH₄ + ₂O₂ → CO₂ + ₂H₂O |
Use these reactions with molar mass calculations when you need the molar mass for each species.
Do You Know?
– Chloromethane contains 3 element types: C, H, Cl.
– Cl contributes the largest share of this compound's total molar mass.
– In C₁H₃Cl, H appears with the highest atom count.
– Its molar mass is 50.48 g/mol, which is used directly in gram-to-mole conversions.
– A common reaction for Chloromethane is synthesis (₂H₂ + O₂ → ₂H₂O).
Why This Compound Matters
Chloromethane 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 Chloroethane (C2H5Cl) and Chloropropane (C3H7Cl).
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 C₁H₃Cl and miscounting atoms.
- Rounding atomic masses too early before finishing all multiplication steps.
- Mixing up Cl element contribution with total molar mass.
- Reporting a value without units; final answer should be in g/mol for Chloromethane.
Quick Revision
Formula: C1H3Cl
Molar Mass: 50.48 g/mol
Key takeaway: count atoms accurately, multiply by atomic masses, and sum only at the end.
Formula Explanation
C1H3Cl contains Carbon (C) (1), Hydrogen (H) (3), Chlorine (Cl) (1). Add each element contribution to get total molar mass.
FAQ
Conclusion
Molar Mass of Chloromethane and Molar Mass of C₁H₃Cl are now easy to revise with this structured page. You can use this method in exams, lab reports, and daily chemistry practice.