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29/12/2020 4:01 pm
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If bromine atom is available in the form of, say two isotopes \(_{35}^{79}{Br}\) (49.70%) and \(_{35}^{81}{Br}\) (50.30%), calculate the average atomic mass of bromine atom.
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29/12/2020 4:07 pm
% of \(_{35}^{79}{Br}\) isotope = 49.7
% of \(_{35}^{81}{Br}\) isotope = 50.3
Average atomic mass of bromine atom
= \(\frac{49.7\times79+ 50.3\times81}{100}\) = \(\frac{3926.3+4074.3}{100}\)
= \(\frac{80006}{1000}\) = 80.006 u