A certain element x has four isotopes. 0.5600% of x has a mass of 83.91343 amu. 9.860% of x has a mass of 85.90927 amu. 7.000% of x has a mass of 86.90890 amu. 82.58% of x has a mass of 87.90562 amu. What is the average atomic mass of element x?

Average Atomic Weight (X) = 87.638974 amu

Explanation:

To find the average atomic weight of an unknown element that exhibit multiple isotopes is given by:

Average Atomic Weight = Percentage of given isotope in the mass spectrum x The corresponding atomic weight of given isotope

Average Atomic Weight (X) = [0.0056 x 83.91343] + [0.098860 x 85.90927] + [0.07 x 86.90890] + [0.8258 x 87.90562] = 87.638974 amu

solution:

Find the average of atomic weight is

(0.0056 x 83.91343) + (0.098860 x 85.90927) + (0.07x86.90890) + (0.8258x87.90562) = 87.61665 amu