9. Element X has two naturally occurring isotopes; 10x with a percent abundance of 85% and 12x with a percent of 15% abundance Which is the most likely average atomic mass for element X? A. 10.1 amu B. 11.9 amu C. 12.3 amu D. 22.0 amu 2
9. Element X has two naturally occurring isotopes; 10x with a percent abundance of 85% and 12x with a percent of 15% abundance Which is the most likely average atomic mass for element X? A. 10.1 amu B. 11.9 amu C. 12.3 amu D. 22.0 amu 2
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Question 9:**
Element X has two naturally occurring isotopes, \(^{10}\text{X}\) with a percent abundance of 85% and \(^{12}\text{X}\) with a percent abundance of 15%. Which is the most likely average atomic mass for element X?
- A. 10.1 amu
- B. 11.9 amu
- C. 12.3 amu
- D. 22.0 amu
*Explanation:*
To determine the most likely average atomic mass, use the formula:
\[
\text{Average atomic mass} = (\text{mass of } ^{10}\text{X} \times \text{abundance of } ^{10}\text{X}) + (\text{mass of } ^{12}\text{X} \times \text{abundance of } ^{12}\text{X})
\]
Convert the percentage abundances into decimal form before calculating.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd208a605-9e71-4cbe-b0c9-a48d8442681c%2F3198431d-7394-4599-8c3d-73a38ab12606%2F49mp5rp_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question 9:**
Element X has two naturally occurring isotopes, \(^{10}\text{X}\) with a percent abundance of 85% and \(^{12}\text{X}\) with a percent abundance of 15%. Which is the most likely average atomic mass for element X?
- A. 10.1 amu
- B. 11.9 amu
- C. 12.3 amu
- D. 22.0 amu
*Explanation:*
To determine the most likely average atomic mass, use the formula:
\[
\text{Average atomic mass} = (\text{mass of } ^{10}\text{X} \times \text{abundance of } ^{10}\text{X}) + (\text{mass of } ^{12}\text{X} \times \text{abundance of } ^{12}\text{X})
\]
Convert the percentage abundances into decimal form before calculating.
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