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Element x has two naturally occurring isotopes. The masses (amu) and % abundance are given. 31x is 35% with mass of 31.16 and 34x is 64% with 34.3 amu's
What are the Weighted Averages of Element X Isotopes: 31x and 34x?
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SUMMARY
The discussion focuses on calculating the weighted average atomic mass of Element X, which has two isotopes: 31x with a mass of 31.16 amu and an abundance of 35%, and 34x with a mass of 34.3 amu and an abundance of 64%. The method for calculating the atomic mass involves using the formula for weighted averages, similar to the example provided for chlorine isotopes (Cl-35 and Cl-37). The calculation for Element X requires multiplying the mass of each isotope by its respective abundance and summing the results.
PREREQUISITES- Understanding of weighted averages
- Knowledge of atomic mass units (amu)
- Familiarity with isotope abundance
- Basic arithmetic operations
- Learn how to calculate weighted averages in chemistry
- Study the concept of isotopes and their significance in atomic mass
- Explore the differences between stable and unstable isotopes
- Investigate the applications of isotopic analysis in scientific research
Chemistry students, educators, and professionals involved in isotopic research or atomic mass calculations will benefit from this discussion.