**Calculating the Average Atomic Mass**A sample of element X has two naturally occurring isotopes. The isotope X-45 makes up 35.8% of the sample, and the isotope X-47 makes up 64.2% of the sample. Calculate the average atomic mass of element X.**Explanation:**To find the average atomic mass of element X, you will need to use the following formula:\[ \text{Average Atomic Mass} = \sum (\text{fractional abundance} \times \text{atomic mass}) \]In this case:- Isotope X-45 has an atomic mass of 45 and makes up 35.8% of the sample.- Isotope X-47 has an atomic mass of 47 and makes up 64.2% of the sample.**Step-by-Step Calculation:**1. Convert the percentages to fractions: - X-45: $\frac{35.8}{100} = 0.358$ - X-47: $\frac{64.2}{100} = 0.642$2. Multiply the fractional abundance by the atomic mass for each isotope: - X-45: $0.358 \times 45 = 16.11$ - X-47: $0.642 \times 47 = 30.174$3. Add these values to get the average atomic mass: - $16.11 + 30.174 = 46.284$Therefore, the average atomic mass of element X is approximately 46.28.This calculation shows how the average atomic mass of an element is derived from the masses and relative abundances of its isotopes.

Isotopes are species having same atomic number but different mass number. Given: The percentage of…

A sample of element X has two naturally occurring isotopes. The isotope X-45 makes up 35.8% of the sample, and the isotope X-47 makes up 64.2% of the sample. Calculate the average atomic mass of element X.

A sample of element X has two naturally occurring isotopes. The isotope X-45 makes up 35.8% of the sample, and the isotope X-47 makes up 64.2% of the sample. Calculate the average atomic mass of element X.

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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