The average atomic mass of a sample of element X is 80 u. It has
Two Naturally Occurring Isotopes X-79 and X-81. What is
the percentage of both the isotopes of element X?
Answers
Answer:
Let the percentage of
8
16
X be A %. Then the percentage of
8
18
X be (100−A) %.
∴ 16×
100
A
+18×
100
100−A
=16.2
⟹1800−2A=1620
⟹A=90
So the answer is 90%
8
16
X and 10%
8
18
X
Explanation:
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Answer:
The percentage of isotope X-79 is 98.75% and ,
the percentage of X-81 is 101.25%.
Explanation:
The average atomic mass of a sample of an element is the weighted average of the atomic masses of its isotopes, where the weights are the abundances of the isotopes. If the average atomic mass of element X is 80 u and it has two isotopes X-79 and X-81, then we can use the following equation to calculate the percentage of each isotope:
% isotope = (atomic mass of isotope) / (average atomic mass) * 100%
For X-79:
% X-79 = (79 u) / (80 u) * 100% = 98.75%
For X-81:
% X-81 = (81 u) / (80 u) * 100% = 101.25%
So, the percentage of X-79 is 98.75% and the percentage of X-81 is 101.25%. Note that these percentages are relative to each other and add up to 100%.
This means that if we have 100 atoms of element X, 98.75 of them will be X-79 and the remaining 101.25 will be X-81. The average atomic mass of the sample will be the weighted average of the atomic masses of the isotopes, considering their abundances. The average atomic mass of the sample, in this case, is 80 u, which is equal to the weighted average of the atomic masses of X-79 and X-81.
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