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The average atomic mass of sample of an element X is 16.2 u. What are the percentages of isotopes \(^{16}_8X\) and \(^{18}_8X\) ?

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Suppose the percentages of \(^{16}_8X\) and \(^{18}_8X\) are Y and 100 - Y .

Average atomic mass = \(\frac{Y}{100}\, \times\,16\,+\,\frac{100\,-\,Y}{100}\,\times\,18\)

16.2 = \(\frac{8Y\,+\,9(100\,-\,Y)}{50}\)

8Y + 900 - 9Y =16.2 x 50

Y = 900 - 810

Y = 90

The percentage of first isotope is 90 and percentage of second isotope is 10.

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