Given the relative abundance of the following naturally occurring isotopes of oxygen: O-16: 99.76%, O-17: 0.037%, and O-18: 0.204%, how would you calculate atomic mass?

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Given the relative abundance of the following naturally occurring isotopes of oxygen: O-16: 99.76%, O-17: 0.037%, and O-18: 0.204%, how would you calculate atomic mass?

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Answer 1 · 2015-10-26T14:15:01

$AAM = \sum (isotope mass \times percent Abundance)$ $"AAM"=sum("isotope mass"xx"percent Abundance")$

Explanation:

The average atomic mass ( $AAM$ $"AAM"$ ) is calculated by the following expression:

$AAM = \sum (isotope mass \times percent Abundance)$ $"AAM"=sum ("isotope mass"xx"percent Abundance")$

Therefore, to calculate the average atomic mass of oxygen:

$AAM = (16 \times 0.9976) + (17 \times 0.00037) + (18 \times 0.00204) = 16.00 a.m.u.$ $"AAM"=(16xx0.9976)+(17xx0.00037)+(18xx0.00204)=16.00 " a.m.u."$

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Given the relative abundance of the following naturally occurring isotopes of oxygen: O-16: 99.76%, O-17: 0.037%, and O-18: 0.204%, how would you calculate atomic mass?

1 Answer

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