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7. An element exists as 3 stable isotopes in nature. The isotopic masses (in amu) and percent abundances are given below. 15.994915 amu 99.757 % 16.999132 amu 0.03800% 17.99916 amu 0.2050 % Determine what the element is by calculating the average atomic mass (in amu). A: O; 15.999 amu

7. An element exists as 3 stable isotopes in nature. The isotopic masses (in amu) and percent abundances are given below. 15.994915 amu 99.757 % 16.999132 amu 0.03800% 17.99916 amu 0.2050 % Determine what the element is by calculating the average atomic mass (in amu). A: O; 15.999 amu

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter2: Atoms, Molecules, And Ions
Section: Chapter Questions
Problem 22E: An element has the following natural abundances and isotopic masses: 90.92% abundance with 19.99...
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The answer should be 0; 15.999 amu
7. An element exists as 3 stable isotopes in nature. The isotopic masses (in amu) and percent abundances are given below. 15.994915 amu 99.757 % 16.999132 amu 0.03800% 17.99916 amu 0.2050 % Determine what the element is by calculating the average atomic mass (in amu). A: O; 15.999 amu
Transcribed Image Text:7. An element exists as 3 stable isotopes in nature. The isotopic masses (in amu) and percent abundances are given below. 15.994915 amu 99.757 % 16.999132 amu 0.03800% 17.99916 amu 0.2050 % Determine what the element is by calculating the average atomic mass (in amu). A: O; 15.999 amu
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