Mg has three natural isotopes whose isotopic masses and relative abundances are respectively 23.98 (78.60%), 24.98(10.11%) and 25.98(11.29%). The atomic mass of Mg will be

Q. 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 ${}_{12}^{24}Mg$ (23.98504u), ${}_{12}^{25}Mg$ (24.98584u) and ${}_{12}^{26}Mg$ (25.98259u). The natural abundance of ${}_{12}^{24}Mg$ is 78.99% by mass. Calculate the abundances of other two isotopes.

Q. What is the average atomic mass of Mg if the naturally occurring isotopes are ${}^{24}Mg$, ${}^{25}Mg$ and ${}^{26}Mg$. Their masses and abundances are as follows:

$\begin{array}{ccc}\text{Isotope}& \text{Atomic Mass}& \text{Isotopic abundance}\\ {}^{24}Mg& 23.98504& 78.70\%\\ {}^{25}Mg& 24.98584& 10.13\%\\ {}^{26}Mg& 25.98259& 11.17\%\end{array}$

Q. Substance $X$ has three common isotopes: $X-48,X-49$ and $X-51$. If the relative abundances of these three isotopes are $42$%, $38$% and $20$% respectively, what is the atomic mass of substance $X$?

Q.

1)carbon has,3 isotopes of atomic mass unit 12. 0 u and 13. 0 u and 14 u the relative abundance of these three isotopes are 98. 8 9 and 1. 10 and 2x10-10 respectively find out the average atomic mass of carbon?

Q. Boron has two isotopes, ${}^{10}B$ and ${}^{11}B$ whose relative abundances are $20$% and $80$% respectively. Atomic weight of boron is: