1. What is Carbon's Atomic Mass?

The atomic mass of carbon is approximately 12.011 g/mol. This value is a weighted average of all naturally occurring isotopes of carbon, primarily carbon-12 (about 98.9%) and carbon-13 (about 1.1%).

2. How Does the Calculator Work?

The calculator uses the simple formula:

Where:

• 12.011 g/mol — Atomic mass of carbon
• Number of Atoms — The quantity of carbon atoms in your sample

3. Importance of Carbon's Atomic Mass

Details: Knowing carbon's atomic mass is fundamental for stoichiometric calculations in chemistry, determining molecular weights of organic compounds, and understanding chemical reactions where carbon is involved.

4. Using the Calculator

Tips: Simply enter the number of carbon atoms you want to calculate the mass for. The calculator will automatically compute the total mass based on carbon's standard atomic weight.

5. Frequently Asked Questions (FAQ)

Q1: Why isn't carbon's atomic mass exactly 12?
A: While carbon-12 is defined as exactly 12 atomic mass units, the natural atomic weight accounts for the presence of other isotopes like carbon-13.

Q2: How precise is this calculation?
A: The calculation uses the IUPAC standard atomic weight of carbon (12.011) which is precise for most practical applications.

Q3: Does this account for different carbon isotopes?
A: The standard atomic weight already accounts for natural isotopic abundance. For specific isotopes, you would need to use their exact masses.

Q4: Can I use this for large quantities of carbon?
A: Yes, the calculator works for any number of atoms, from single atoms to Avogadro's number (6.022×10²³ atoms = 1 mole).

Q5: How does this relate to molar mass?
A: The atomic mass in g/mol is numerically equal to the molar mass, so 12.011 g of carbon contains approximately 1 mole of carbon atoms.