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tangare [24]
3 years ago
7

The element chlorine has two stable isotopes, chlorine-35 with a mass of 34.97 amu and chlorine-37 with a mass of 36.95 amu. Fro

m the atomic weight of Cl = 35.45 one can conclude that:
Chemistry
1 answer:
sergejj [24]3 years ago
7 0

<u>Answer: </u>One isotope has a percentage abundance of 75.75 % and the percentage abundance of another isotope is 24.24%.

<u>Explanation:</u>

We are given the two stable isotopes of chlorine with their respective masses. The average atomic mass of chlorine is also given.

Average atomic mass of chlorine = 35.45 amu.

Let us assume the fractional abundance of one isotope be 'x' and the fractional abundance for another isotope will be (1 - x) because the total fractional abundance is always equal to 1.

  • For Chlorine-35 isotope:

Fractional abundance = x

Mass = 34.97 amu

  • For Chlorine-37 isotope:

Fractional abundance = 1 - x

Mass = 36.95 amu

The formula for the calculation of average atomic mass is given by:

\text{Average atomic mass }=\sum_{i=1}^n\text{(Atomic mass of an isotopes)}_i\times \text{(Fractional abundance})_i

Putting values in above equation, we get:

35.45=34.97(x)+36.95(1-x)\\\\35.45=34.97x+36.95-36.95\\\\-1.5=-1.98x\\\\x=\frac{-1.5}{-1.98}=0.7575

1-x=1-0.7575=0.2424

Converting these two fractional abundances into percentage abundances by multiplying it with 100.

x=0.7575\times 100=75.75\%\\\\1-x=0.2424\times 100=24.24\%

Hence, one isotope has a percentage abundance of 75.75 % and the percentage abundance of another isotope is 24.24%.

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