Question

"Naturally occurring boron is composed of two isotopes. The percent abundance and the mass of each isotope are listed below: 19.9% of boron atoms have a mass of 10.013 amu, and 80.1% of the boron atoms have a mass of 11.009 amu. To calculate the average atomic mass of boron, you would set up the following calculation: What is the average atomic mass of boron?"

To calculate the average atomic mass, you would use a weighted average based on the percent abundance of each isotope. If you need help with the specific calculation, please let me know.

Answer 1

To calculate the average atomic mass of boron, you would use a weighted average based on the percent abundance of each isotope.

Step-by-step explanation:

To calculate the average atomic mass of boron, you would use a weighted average based on the percent abundance of each isotope. The percent abundance of each isotope is given in the question: 19.9% for boron-10 and 80.1% for boron-11. To calculate the average atomic mass, you would multiply the mass of each isotope by its percent abundance, and then add these values together.

For boron-10: (0.199) * (10.013 amu) = 1.993 amu

For boron-11: (0.801) * (11.009 amu) = 8.827 amu

Adding these values together: 1.993 amu + 8.827 amu = 10.82 amu

Therefore, the average atomic mass of boron is 10.82 amu.