What is the average atomic mass of chlorine if it has isotopes of masses 36.96590 and 34.96885, which are 24.47% and 75.53% abundant, respectively?

Aug 20, 2017

The average atomic mass of the given sample of chlorine is $\text{35.46 u}$.

Explanation:

Change the percentages to their decimal forms:

24.47%=24.47/100=0.2447

75.53%=75.53/100=0.7553

Multiply the mass of each isotope by its percent abundance and add. The symbol $\text{u}$ is used for atomic mass units.

$\text{0.2447(36.9590 u)+0.7553(34.96885 u)"="35.46 u}$

Aug 20, 2017

$35.4573$

Explanation:

The average mass is summation of the percentages of each mass multiplied by that mass.
$\left(36.9650 \times 0.2447\right) + \left(34.96885 \times 0.7553\right) = 35.4573$