A hypothetical element x has 3 naturally occurring isotopes: 41.20% of 21x, with an atomic weight of 21.016 amu, 50.12% of 22x,

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A hypothetical element x has 3 naturally occurring isotopes: 41.20% of 21x, with an atomic weight of 21.016 amu, 50.12% of 22x,

with an atomic weight of 21.942 amu, and 8.68% of 24x, with an atomic weight of 23.974 amu. on the basis of these data, calculate the average atomic weight of element x. report your answer to two decimal places.

Chemistry

1 answer:

iogann1982 [59] · Answer 1 · 2022-02-24T10:33:40+03:00

The average atomic weight is calculated by adding up the products of the percentage abundance and atomic weight. In this item, we have the equation,

A = (0.412)(21.016 amu) + (0.5012)(21.942 amu) + (0.0868)(23.974 amu)

Simplifying the operation will give us the answer of 21.74 amu.

<em>Answer: 21.74 amu</em>