SUMMARY
The discussion focuses on calculating the apparent atomic mass of a contaminated iodine sample. The naturally occurring iodine has an atomic mass of 126.9045 g/mol, while the synthetic radioisotope, 129I, has an atomic mass of 128.9050 g/mol. Given a 12.3849 g sample of iodine contaminated with 1.00070 g of 129I, the calculation involves determining the weighted average of the isotopes based on their respective masses and proportions. This method is essential for accurately assessing the atomic mass in the presence of isotopic contamination.
PREREQUISITES
- Understanding of atomic mass and isotopes
- Knowledge of weighted averages in chemistry
- Familiarity with basic mass measurement techniques
- Basic algebra for calculations
NEXT STEPS
- Study the concept of weighted averages in chemistry
- Learn about isotopic composition and its effects on atomic mass
- Explore the properties and applications of iodine isotopes
- Investigate the calculation methods for atomic mass in contaminated samples
USEFUL FOR
Chemistry students, educators, and professionals involved in nuclear medicine or isotopic analysis will benefit from this discussion.