A certain element consists of two stable isotopes. The first has a mass of 14.0 amu and a percent natural abundance of 99.6 %. The second has a mass of 15.0 amu and a percent natural abundance of 0.370 %. What is the atomic weight of the element? amu
A certain element consists of two stable isotopes. The first has a mass of 14.0 amu and a percent natural abundance of 99.6 %. The second has a mass of 15.0 amu and a percent natural abundance of 0.370 %. What is the atomic weight of the element? amu
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter2: Atoms Molecules And Ions
Section: Chapter Questions
Problem 164SCQ
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The atomic weight of the element with isotope mass and its abundance is calculated using the formula
Where fractional abundance is calculated by dividing percent abundance by 100.
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