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.

Question

Joel Buchanan

Chemistry

26 February, 08:48

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.

+3

Answers (1)

Know the Answer?

Zayden Joyce · Answer 1

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.

Answer: 21.74 amu