The isotopes of an element have mass numbers A, A + 1, A + 2. The ratio of abundance of these isotopes is $3:2:4$. Calculate the average atomic mass of the element.:

Q. An element has average atomic mass $20.426u$ it has $2$ isotopes with masses $22.1824$ and $19.9574$. Calculate the abundance of its isotopes $X-22$ and $X-20$.

Q. An element has four isotopes, each differing by an atomic mass of 1. The ratio of their abundance from the lightest to heaviest isotope is 1:2:2:3, respectively. Determine the average atomic mass of the element, if the mass of the heaviest isotope is A.

Q. Mass numbers of two isotopes of an element differ by $2$ units ($A$ and $A+2$). Average atomic mass is $0.5$ more than the lower mass number. What could be the ratio of the percentage abundance two isotopes respectively?

Q. Mass numbers of two isotopes of an element differ by 2 units (A and A+2). Average atomic mass is 0.5 more than the lower mass number. What could be the ratio of the percentage abundance two isotopes respectively?

Q. The ratio of the mass of ${}^{12}C$ atom to that of an atom of element= X (whose atomicity is four) is 1:9. The molecular mass element X is: