Answer:
Step-by-step explanation:
The atomic mass of each stable isotope of carbon found in nature is as follows:
1. Carbon-12 (C-12):
- Isotope symbol: 12/6C
- Natural % abundance: 98.89%
- Atomic mass: 12 atomic mass units (amu)
2. Carbon-13 (C-13):
- Isotope symbol: 13/6C
- Natural % abundance: 1.11%
- Atomic mass: 13 amu
In nature, carbon exists as a mixture of these two isotopes, with Carbon-12 being the most abundant. The atomic mass of an element is determined by the weighted average of the atomic masses of its isotopes, taking into account their relative abundances. Therefore, the average atomic mass of carbon, considering these two isotopes and their natural abundances, is approximately 12.01 amu.