The relative atomic mass of element X is 41.4 amu while the relative atomic mass of the second element is 162.3 amu
The questions are incomplete, the complete questions are;
1) Element X has three naturally occurring isotopes. The mass (amu) and % abundance of the isotopes are 37.919 amu (5.07%), 39.017 amu (15.35%), and 42.111 amu (79.58%). What is the average atomic mass of element X?
2) A certain element has three isotopes. The isotopic masses and abundances are: 159.37 amu (30.60%), 162.79 amu (15.79%), and 163.92 amu (53.61%). What is the average atomic weight of the element?
We can obtain the average atomic mass the the sum of the products of relative abundance and isotope mass for all the isotopes of the element.
Note that isotopes of an element has different masses and abundances. The average atomic mass of the element includes contribution from all these isotopes.
1) (37.919 × 0.0507) + (39.017 × 0 .1535) + (42.11 × 0.7958) = 41.4 amu
2) (159.37 × 0.3060) + (162.79 × 0.1579) + (163.92 ×0 .5361) = 162.3 amu
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