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in a sample of silcon 92.21% of the atoms have a mass of 27.98 amu, 4.70% have a mass of 28.98 amu and 3.09% have a mass of 29.97 amu. what is ther average atomic mass of the sample? socratic.org socratic.org

User Mike Koder
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1 Answer

1 vote

Answer: 28.1 amu

Step-by-step explanation:

Mass of isotope 1 = 27.98 amu

% abundance of isotope 1 = 92.21% =
(92.21)/(100)=0.9221

Mass of isotope 2 = 28.98 amu

% abundance of isotope 2 = 4.70% =
(4.70)/(100)=0.047

Mass of isotope 3 = 29.97 amu

% abundance of isotope 2 = 3.09% =
(3.09)/(100)=0.0309

Formula used for average atomic mass of an element :


\text{ Average atomic mass of an element}=\sum(\text{atomic mass of an isotopes}* {{\text { fractional abundance}})


A=\sum[(27.98 )* 0.922+(28.98)* 0.047+(29.97)* 0.0309]


A=28.1amu

Therefore, the average atomic mass of silicon is 28.1 amu

User Cooper Scott
by
7.7k points
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