A fictional element named Schwartzium is found to have two naturally occurring isotopes with the natural abundances shown here:          Mass (amu)         % Abundance           32.3456                   65%           31.7812                   35% The calculated atomic mass (in amu) of Schwartzium is (place only a numerical answer, no units, in the following box):Group of answer choices32.3456 amu31.7812 amu31.9787 amu32.1481 amuinsufficient information provided to answer question

A fictional element has two naturally occurring isotopes with the natural abundances shown here: ATOMIC MASS (AMU) ABUNDANCE1650.0%1850.0% Which statement is TRUE for this element?Group of answer choicesThe atomic mass would be 16.The atomic mass would be less than 16.The atomic mass would be 18.The atomic mass would be more than 18.The atomic mass would be 17.

An element X has four naturally occurring isotopes, with natural abundances and masses outlined in the table below. Mass (a.m.u) Natural Abundance (%)21.00 45.50 %23.00 32.00 %24.00 12.60 %26.00 9.90 %Calculate the atomic mass of element X, to two decimal places.

The isotopic masses (amu) and % abundances of the isotopes are given below. Isotope Abundance (%) Mass (amu)159X 30.60 159.37163X 15.79 162.79164X  53.61 163.92 The average atomic mass of the element is __________ amu.Question 1Select one:a.161.75b.162.03c.162.35d.163.15e.33.33

The average atomic mass of Re is 186.207 amu. It is calculated from the two naturally occurring isotopes 185Re and 187Re. If the isotopic abundance of 185Re is 37.4% and the isotopic mass of 185Re is 184.953 amu calculate the mass of 187Re.Group of answer choices

lement X has two isotopes. Their mass numbers are 69 and 71 The percentage abundance of each isotope is: • 60% of 69 X • 40% of 71 X Estimate the relative atomic mass of element X. [1 mark] Tick one box. < 69.5 Between 69.5 and 70.0 Between 70.0 and 70.5 > 70.5