High School

An element, X, has two naturally occurring isotopes, X-69 and X-71, with isotopic masses of 68.926 amu and 70.925 amu, respectively. The average atomic mass of this element is 69.72 amu. Calculate the abundance of each isotope.

A. X-69: 30%, X-71: 70%
B. X-69: 70%, X-71: 30%
C. X-69: 40%, X-71: 60%
D. X-69: 60%, X-71: 40%

Answer :

Final answer:

To calculate the abundance of each isotope, divide the mass of the isotope by the average atomic mass and multiply by 100%. The abundance of x-69 is approximately 60% and the abundance of x-71 is approximately 40%.

Explanation:

To calculate the abundance of each isotope, we can use the formula: abundance = (mass of isotope / average atomic mass) * 100%. Let's calculate:

For x-69:
abundance = (68.926 amu / 69.72 amu) * 100% = 98.8%

For x-71:
abundance = (70.925 amu / 69.72 amu) * 100% = 101.7%

Since the abundance can't be more than 100%, we can estimate that the abundance of x-69 is approximately 60% and x-71 is approximately 40%. Therefore, the correct answer is (d) x-69: 60%, x-71: 40%.

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