A particular element found in nature exists as two stable isotopes. 60.4% of the element has a mass of 68.9257amu, the rest of the element is found with a mass of 70.9249 amu. Calculate the average atomic mass of the element.
mass %abundance # of atoms (pick 1000 sample) 68.9257 60.4% 604 70.9249 39.6% 396 *39.6* ( i got this by subtracting 100 as most percentage is out of 100) *# of atoms* ( i just moved it one decimal place, then i am going to make the sample out of 1000, to get the decimal place) Formula= total mass/ total #atoms x= (68.9257u* 604) + (70. 9249*396)/ 1000 x- 69717. 3832/ 1000 x= 69.717amu or 69.72 amu if you look on the periodic table the closet element with that mass is gallium ( amu is 69.72)