Try the fastest way to create flashcards
Question

An element has two naturally occurring isotopes. The isotope has a mass of 62.9396 amu and a relative abundance of 69.17 %, and isotope 2 has a mass of 64.9278 amu.

Find the atomic mass of this element.

Solution

Verified
Answered 9 months ago
Answered 9 months ago
Step 1
1 of 4

To calculate the atomic mass of this element we have to calculate the average mass of these two isotopes.

Since this element has 2 occurring isotopes it means that the isotope 1 and 2 make up 100% of the abundance.

Create a free account to view solutions

Create a free account to view solutions

Recommended textbook solutions

Chemistry: The Molecular Nature of Matter and Change 7th Edition by Patricia Amateis, Silberberg

Chemistry: The Molecular Nature of Matter and Change

7th EditionISBN: 9780073511177 (2 more)Patricia Amateis, Silberberg
6,032 solutions
Chemistry: The Central Science 14th Edition by Bruce Edward Bursten, Catherine J. Murphy, H. Eugene Lemay, Matthew E. Stoltzfus, Patrick Woodward, Theodore E. Brown

Chemistry: The Central Science

14th EditionISBN: 9780134414232 (9 more)Bruce Edward Bursten, Catherine J. Murphy, H. Eugene Lemay, Matthew E. Stoltzfus, Patrick Woodward, Theodore E. Brown
7,736 solutions
Atkins' Physical Chemistry 11th Edition by James Keeler, Julio de Paula, Peter Atkins

Atkins' Physical Chemistry

11th EditionISBN: 9780198769866James Keeler, Julio de Paula, Peter Atkins
1,692 solutions
Modern Chemistry 1st Edition by Jerry L. Sarquis, Mickey Sarquis

Modern Chemistry

1st EditionISBN: 9780547586632 (2 more)Jerry L. Sarquis, Mickey Sarquis
2,184 solutions

More related questions

1/4

1/7