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hram777 [196]
3 years ago
11

An element has two naturally-occurring isotopes. The mass numbers of these isotopes are 113 amu and 115 amu, with natural abunda

nces of 5% and 95%, respectively. Calculate its average atomic mass. Report your answer to 1 decimal place.
Chemistry
1 answer:
DENIUS [597]3 years ago
5 0

Answer: Its average atomic mass is 114.9 amu

Explanation:

Mass of isotope 1 = 113 amu

% abundance of isotope 1 = 5% = \frac{5}{100}=0.05

Mass of isotope 2 = 115 amu

% abundance of isotope 2 = 95% = \frac{95}{100}=0.95

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[(113\times 0.05)+(115\times 0.95)]

A=114.9amu

Thus its average atomic mass is 114.9 amu

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