Question

Enter your answer in the provided box. An element has two naturally occurring isotopes. The mass numbers of these isotopes are 109 amu and 111 amu, with natural abundances of 35% and 65%, respectively. Calculate its average atomic mass. Report your answer to 1 decimal place. amu

Answer 1

Given data's Isotopes = log amy mass number mass number of of first second isotopes = 111 amy first isotopes = 3 % Natural abundance of Matural abundame of second isotopes = 65% Average atomic mass = (mass number of first Isotopes x natural abundance of first Isotopes It (mass number of second isotopes & natural abundance of second isotopes Average atomic mass = (logamu x 0.35) + ( 111 amy xooos! = 38.15amu + 72.15ama Average atomic mass = 110.30 amu Scanned with CamScanner