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vivado [14]
3 years ago
14

What is the average isotopic mass of an element that has the following abundances in nature? Isotopic mass: X20 X22 X23 Abundanc

es in natures: 90.5 % 8.0 % 1.5 %
Chemistry
1 answer:
Paladinen [302]3 years ago
8 0

Answer: 20.2

Explanation:

Mass of isotope 1 = 20

% abundance of isotope 1 = 90.5% = \frac{90.5}{100}=0.905

Mass of isotope 2 = 22

% abundance of isotope 2 = 8.0% = \frac{8}{100}=0.08

Mass of isotope 3 = 23

% abundance of isotope 3 = 1.5% = \frac{1.5}{100}=0.015

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[(20\times 0.905+(22\times 0.08)+(23\times 0.015]

A=20.2

Therefore, the average atomic mass of the element is 20.2.

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