" Two isotopes of an element (atomic mass "=x+2.35" ) have mass "(x+2)" and "(x+7)" respectively.Calculate natural abundance of heavier isotope in percentage."

Isotopes have same number of atomic mass

There are two isotopes of an element with atomic mass z. Heavier on has atomic mass z+2 and lighter one has z-1, then abundance of lighter one is

The relative abundance of two isotopes of an element with atomic weight 85 and 87 is 75% and 25% respectively. Then calculate the average atomic weight of element

Chlorine consists of the two isotopes ""_(17)Cl^(35) and "'_(17)Cl^(37) of masses 34.99 amu and 36.97 amu, respectively. Calculate the relative abundance of each isotope if atomic mass of chlorine is 35.46 amu.

The natural lithium is composed of two isotopes of ""_(3)Li^(6) and ""_(3)Li^(7) . The isotopes have masses 6.015121 amu and 7.016003 amu, respectively. Calculate the relative abundance of each isotope in the natural lithium if the atomic mass of natural lithium is 6.94 amu.

Lithium exists in nature in the form of two isotopes, Li-6 and Li-7 with atomic masses 6.0151u and 7.0160u and the percentages 8.24 and 91.76 respectively. Calculate average atomic mass.

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.

The element bron occurs in nature as two isotopes havein atomic masses 10 u and 11 u . What are the percentage abundances of these isotopes in a sample of boron having average atomic mass of 10.8 u?