What is the average atomic mass of an element composed of a series of isotopes, $X, Y, Z$ $X, Y, Z$ with respective masses, $18.473 \cdot amu, 19.962 \cdot amu, 21.469 \cdot amu$ $18.473"amu", 19.962"amu", 21.469*"amu"$ , and respective abundances, $X = 28.812 %$ $X=28.812%$ , $Y = 28.757 %$ $Y=28.757%$ ...?

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What is the average atomic mass of an element composed of a series of isotopes, $X, Y, Z$ $X, Y, Z$ with respective masses, $18.473 \cdot amu, 19.962 \cdot amu, 21.469 \cdot amu$ $18.473"amu", 19.962"amu", 21.469*"amu"$ , and respective abundances, $X = 28.812 %$ $X=28.812%$ , $Y = 28.757 %$ $Y=28.757%$ ...?

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Answer 1 · 2018-02-07T21:40:29

We take the weighted average ..... and get $20.15 \cdot amu$ $20.15*"amu"$

Explanation:

$Average atomic mass = {{18.473}_{X} \times 28.812 % + {19.962}_{Y} \times 28.757 % + {21.469}_{Z} \times (100 - 28.812 - 28.757) %} \cdot amu$ $"Average atomic mass"={18.473_"X"xx28.812%+19.962_"Y"xx 28.757% +21.469_"Z" xx(100-28.812-28.757)%}*"amu"$

$\equiv 20.15 \cdot amu$ $-=20.15*"amu"$ ...if I have done my 'rithmetic right...

How did I get the percentage abundance of $Z$ $Z$ ?

And it is likely that we got the element neon. How did I know this?

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What is the average atomic mass of an element composed of a series of isotopes, X,Y,ZX, Y, Z with respective masses, 18.473⋅amu,19.962⋅amu,21.469⋅amu18.473*"amu", 19.962*"amu", 21.469*"amu", and respective abundances, X=28.812%X=28.812%, Y=28.757%Y=28.757%...?

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Explanation:

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