Calculation of average atomic mass — task. Chemistry CBSE Live product, Class 9.

Calculate the average atomic mass of an element from its isotopes:

If chlorine atom is available in the form of, say, two isotopes, $_{17}\textrm{Cl}^{35}$ ($75.77$%) and $_{17}\textrm{Cl}^{37}$ ($24.23$%), calculate the average atomic mass of chlorine.

The formula to find average atomic mass is

\frac{\sum (Mass of isotopes \times % Natural abundance)}{100}

\frac{\sum (Mass of isotopes \times 100)}{% Natural abundance}

\frac{(% Natureal abundance \times 100)}{\sum (Mass of isotopes)}

d. $\frac{\sum (Mass of isotopes)}{100}$

When substituting the given values in the formula, we get,

$30.5 u$
$35.47 u$
$34.47 u$
$37.5 u$

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8. Calculation of average atomic mass

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