[" Q."6" of has two isotopes "Ne^(20)" and "Ne^(22)" .If atomic weight "],[" the isotopes is the ratio of the relative abundances of "]

The element, boron has two isotopes ( ""^(10)B and ""^(11)B ). Calculate the natural abundance o the isotopes of boron if the atomic mass of the element be 10.8.

An element is found in nature in two isotopic forms with mass numbers (A-1) and (A+3). If the average atomic mass of the element is found to be A, then the relative abundance of the heavier isotope in the nature will be :

An element is found in nature in two isotopic forms with mass numbers (A-1) and (A+3). If the average atomic mass of the element is found to be A, then the relative abundance of the heavier isotope in the nature will be :

An element A exist in two isotopic forms A^15 and A^16 . If the average atomic mass of A was found to be 15.24, then the % relative abundance of A^15 will be

Boron has two isotopes, B-10 and B-11. The average atomic mass of boron is found to be 10.80u. Calculate the percentage of abundance of these isotopes.

Boron has two isotopes, B-10 and B-11. The average atomic mass of boron is found to be 10.80u. Calculate the percentage of abundance of these isotopes.

Boron has two isotopes, B-10 and B-11. The average atomic mass of boron is found to be 10.80u. Calculate the percentage of abundance of these isotopes.