In a periodic table the average atomic mass of magnesium is given as 24.312 u. The average value is based on their relative natural abundance on earth. The three isotopes and their masses are 1224Mg (23.98504u), 1225Mg (24.98584u) and 1226Mg (25.98259u). The natural abundance of 1224Mg is 78.99% by mass. Calculate the abundances of other two isotopes.

Question

In a periodic table the average atomic mass of magnesium is given as 24.312 u. The average value is based on their relative natural abundance on earth. The three isotopes and their masses are 1224​Mg (23.98504u), 1225​Mg (24.98584u) and 1226​Mg (25.98259u). The natural abundance of 1224​Mg is 78.99% by mass. Calculate the abundances of other two isotopes.

Filo · Accepted Answer

Let, the abundance of 12​Mg25 by mass be x%.Therefore, abundance of 12​Mg26 by mass=(100−78.99−x)%=(21.01−x)%Now, average atomic mass of Mg is 24.312=23.98504×10078.99​+24.98584×100x​+25.98259×10021.01−x​⟹x=9.303% for 12​Mg25(21.01−x)% =11.71% for 12​Mg26

Question Text	In a periodic table the average atomic mass of magnesium is given as 24.312 u. The average value is based on their relative natural abundance on earth. The three isotopes and their masses are $_{12}^{24} M g$ (23.98504u), $_{12}^{25} M g$ (24.98584u) and $_{12}^{26} M g$ (25.98259u). The natural abundance of $_{12}^{24} M g$ is 78.99% by mass. Calculate the abundances of other two isotopes.
Answer Type	Text solution:1
Upvotes	150

Text solutionVerified

Practice questions from similar books