Solution: For isotopes 1H, % of natural abundance =99.985 Similarly, for isotopes 2H, % of natural abundance =0.015
Formula used:
Here, A denotes Abundance
Average atomic mass =
(A(1H)
Average atomic mass = ( (99.985×1) + (0.015×2)) / (100)Average atomic mass = 1.00015 uHence, the average atomic mass of H comes out to be 1.00015 u
Hence, from the above solution it is concluded that the average atomic mass of H comes out to be 1.00015 u.