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Question
If bromine atom is available in the form of, say, two isotopes `""_35^79Br (49.7%)" and """_35^81Br (50.3%)`, calculate the average atomic mass of bromine atom.
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Solution
It is given that two isotopes of bromine are `""_35^79Br (49.7%)" and """_35^81Br (50.3%)`
Then, the average atomic mass of the bromine atom is given by:
= `79xx(49.7/100)+81xx(50.3/100)`
= `3926.3/100+4074.3/100`
= `8000.6/100`
= 80.006 u
= 80 u (approx)
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