The question "How to find the molecular mass of carbon?" is slightly misleading since carbon typically exists as a single atom (C) rather than a molecule. However, we can clarify this and answer the implied question: How to determine the atomic mass of carbon and, how the concept of atomic mass relates to molecular mass.
Understanding Atomic Mass and Molecular Mass
According to reference 1, molecular mass is the sum of the atomic masses of all atoms in a molecule. However, the question focuses on carbon, which usually doesn't exist alone as a molecule (like C2 or C3). Instead, we commonly refer to its atomic mass.
Reference 2 gives us the necessary information that the atomic mass of carbon is 12 u. The unit "u" stands for atomic mass units, also sometimes referred to as daltons (Da).
Calculating Molecular Mass: An Example
While carbon's atomic mass is simply 12 u, let's use Reference 3 to demonstrate how molecular mass is calculated using the atomic mass. The reference uses carbon dioxide (CO2) as an example:
| Element | Atomic Mass (u) | Number of Atoms | Calculation |
|---|---|---|---|
| Carbon (C) | 12 | 1 | 1 x 12 = 12 |
| Oxygen (O) | 16 | 2 | 2 x 16 = 32 |
| Total for CO2 | 12 + 32 = 44 u |
As shown in the table, the molecular mass of carbon dioxide (CO2) is calculated by adding the atomic mass of carbon (12 u) to twice the atomic mass of oxygen (2 x 16 u), resulting in a total of 44 u.
Key Points to Remember
- Atomic mass of carbon (C): 12 u
- Molecular mass: The sum of the atomic masses of all atoms within a molecule.
- Carbon's usual form: Carbon generally exists as single atoms, therefore we consider its atomic mass.
- When carbon is in a compound (such as CO2), its atomic mass of 12u is used in the calculation of the compound's molecular mass.
Conclusion
In summary, while the term "molecular mass of carbon" is usually not applied because carbon atoms generally exist individually, its atomic mass is 12u. The concept is best used for molecules made of more than one atom.
