Atomic weight of Ne is 20.2. If Ne is a mixtu | vedclass

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(A) Let the percentage abundance of $Ne^{20}$ be $x$ and that of $Ne^{22}$ be $(100 - x)$.Using the formula for average atomic mass:$Average \ Atomic

Vedclass · Accepted Answer

$90$

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(A) Let the percentage abundance of $Ne^{20}$ be $x$ and that of $Ne^{22}$ be $(100 - x)$.Using the formula for average atomic mass:$Average \ Atomic \ Mass = \frac{(Mass_1 	imes Abundance_1) + (Mass_2 	imes Abundance_2)}{100}$$20.2 = \frac{(20 	imes x) + (22 	imes (100 - x))}{100}$$2020 = 20x + 2200 - 22x$$2020 = 2200 - 2x$$2x = 2200 - 2020$$2x = 180$$x = 90$Thus,the percentage abundance of the lighter isotope $Ne^{20}$ is $90\%$.

Atomic weight of $Ne$ is $20.2$. If $Ne$ is a mixture of $Ne^{20}$ and $Ne^{22}$,what is the percentage abundance of the lighter isotope?

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