A hypothetical element, M, has four stable isotopes with the masses shown below. 109M = 108.9842 amu 107M = 106.9085 amu 105M = 104.9904 amu 103M = 102.9991 amu If the percentage abundance of 109M is 10.5%, 105M is 6.6% and the average atomic mass of M is 106.6785 amu, then what is the percentage abundance for 103M? Enter your answer as a percentage but without the % symbol. Use one decimal place.
A hypothetical element, M, has four stable isotopes with the masses shown below. 109M = 108.9842 amu 107M = 106.9085 amu 105M = 104.9904 amu 103M = 102.9991 amu If the percentage abundance of 109M is 10.5%, 105M is 6.6% and the average atomic mass of M is 106.6785 amu, then what is the percentage abundance for 103M? Enter your answer as a percentage but without the % symbol. Use one decimal place.
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
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
Section2.2: Isotopes And Atomic Weight
Problem 2.3CYU: Neon has three stable isotopes, one with a small abundance. What are the abundances of the other two...
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A hypothetical element, M, has four stable isotopes with the masses shown below.
109M = 108.9842 amu
107M = 106.9085 amu
105M = 104.9904 amu
103M = 102.9991 amu
If the percentage abundance of 109M is 10.5%, 105M is 6.6% and the
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