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.
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 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)
Is there an error in this question or solution?
Solution If bromine atom is available in the form of, say, two isotopes 79 35Br(49.7%) and 81 35Br(50.3%), calculate the average atomic mass of bromine atom. Concept: Structure of Atom Introduction.
