A hypothetical element, Rz, has two isotopes: ¹⁶⁹Rz = 168.94 amu and ¹⁷¹Rz = 170.98 amu. Eleven of every fifteen atoms of Rz found in nature exist as the ¹⁶⁹Rz isotope. What is the average atomic mass of the element Rz?

Question

Quizplus · Accepted Answer

The average atomic mass of Rz is calculated by taking the weighted average of its isotopes based on their natural abundance. With 11 out of 15 atoms being the 168.94 amu isotope, and the remaining 4 being the 170.98 amu isotope, the calculation is as follows: [(11/15) * 168.94] + [(4/15) * 170.98] = 169.48 amu.

A Hypothetical Element, Rz, Has Two Isotopes: 169Rz = 168

A Hypothetical Element, Rz, Has Two Isotopes: ¹⁶⁹Rz = 168