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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

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Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Back Submit Answer References Use the References to access important values if needed for this question. 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? O. Atomic Weight: This is group attempt 2 of 10 Autosaved at 10:50 PM amu
Transcribed Image Text:Back Submit Answer References Use the References to access important values if needed for this question. 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? O. Atomic Weight: This is group attempt 2 of 10 Autosaved at 10:50 PM amu
Expert Solution
Step 1

The atomic weight of the element with isotope mass and its abundance is calculated using the formula

Atomic weight=isotope mass1×fractional abundance1+isotope mass2×fractional abundance2+....

Where fractional abundance is calculated by dividing percent abundance by 100.

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