SUMMARY
The mass of a carbon atom is accurately expressed as 12 atomic mass units (amu) and 1.9924 x 10^-23 grams. This equivalence is derived from the fact that 6.023 x 10^23 atoms of carbon weigh 12 grams, leading to the calculation that one carbon atom weighs 12 amu. Additionally, the conversion to grams confirms that one carbon atom weighs 1.9924 x 10^-23 grams, validating both measurements as correct representations of carbon's atomic mass.
PREREQUISITES
- Understanding of atomic mass units (amu)
- Familiarity with Avogadro's number (6.023 x 10^23)
- Basic knowledge of unit conversion between grams and amu
- Concept of atomic structure and mass measurement
NEXT STEPS
- Research the significance of Avogadro's number in chemistry
- Learn about the concept of atomic mass and its applications
- Explore the relationship between mass and moles in chemical calculations
- Study unit conversion techniques in scientific measurements
USEFUL FOR
Chemistry students, educators, and anyone interested in understanding atomic mass and its implications in chemical calculations.