Question

Please help :’)

Element X has two naturally occurring isotopes ^10X with a percentage abundance of 85% and ^12X with a percentage of 15% abundance. Which is the most likely average atomic mass for Element X?

10.1 amu

11.7 amu

12.3 amu

22.0 amu

Answer 1

Answer:

10*0.85 + 12*0.15 = 10.3 amu

the most likely one will be 10.1 amu.

Hope that helps!

Answer 2

The average atomic mass of the element X is 11.7 amu

Explanation:

Mass of isotope 1 = 10 amu

% abundance of isotope 1 = 15% = $\frac{15}{100}=0.15$

Mass of isotope 2 = 12 amu

% abundance of isotope 2 = 85% = $\frac{85}{100}=0.85$

Formula used for average atomic mass of an element :

$\text{ Average atomic mass of an element}=\sum(\text{atomic mass of an isotopes}\times {{\text { fractional abundance}})$

$A=\sum[(10\times 0.15)+(12\times 0.85)]$

$A=11.7amu$

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