Question

The average mass of a nitrogen atom is 14.006 amu from the two isotopes with the following data: 14N-14.00307 amu with 0.9963 fractional abundance; 1SN- 15.000108 amu with 0.00364 fractional abundance. Calculate the percentage abundance of each isotopic form. Select the correct answer below: a. 13.95% and 0.05%, respectively b. 0.054% and 0.638%, respectively c. 9.63% and 0.0364%, respectively d. 99.63% and 0.364%, respectively

Answer 1

Answer:

d. 99.63% and 0.364%, respectively

Explanation:

The average mass of a nitrogen atom is 14.006 amu

14N-14.00307 amu with 0.9963 fractional abundance

1SN- 15.000108 amu with 0.00364 fractional abundance.

The relative abundance definition in chemistry is the percentage of a particular isotope that occurs in nature. The atomic mass listed for an element on the periodic table is an average mass of all known isotopes of that element.

In this problem, the fractional abundance has areaady been given. All we need to do now is convert them to percentage abundance.

14N-14.00307 = 0.9963* 100% = 99.63%

1SN- 15.000108 = 0.00364 * 100% = 0.364%