Copper has two naturally occurring isotopes. Cu-63 has a mass of 62.939 amu and relative abundance of 69.17%. Use the atomic weight of copper to determine the mass of the other copper isotope.
To calculate the atomic weight, the atomic weight of each isotope is multiplied by its percent abundance (expressed as a decimal). Then the results are added together.
i.e. atomic mass=sum of ((isotopic abundance) (atomic mass)-----(1)
Atomic mass of the element copper = 63.5amu
Atomic mass of first isotope=62.939amu
Relative abundance of second isotope=100-69.17=30.83%
Atomic mass of second isotope is to be found .Let it be x
Substituting the given values in -(1)
63.5amu= 62.939amu 0. 69+30.83x
Mass of the isotope will be 64.93 amu
Textbook: Introductory Chemistry
Author: Nivaldo J Tro
Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. The full step-by-step solution to problem: 106P from chapter: 4 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. This full solution covers the following key subjects: copper, mass, abundance, AMU, determine. This expansive textbook survival guide covers 19 chapters, and 2046 solutions. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. The answer to “Copper has two naturally occurring isotopes. Cu-63 has a mass of 62.939 amu and relative abundance of 69.17%. Use the atomic weight of copper to determine the mass of the other copper isotope.” is broken down into a number of easy to follow steps, and 33 words. Since the solution to 106P from 4 chapter was answered, more than 651 students have viewed the full step-by-step answer.