The average atomic mass of nitrogen is 14.0067. The atomic masses of the two stable isotopes of nitrogen.^14 N and^15 N, are 14.003074002 and 15.00010897 amu, respectively. Use this information to determine the percent abundance of^14 N. % Determine the percent abundance of^15 N. %

The answer to your question is Abundance N-14 = 99.63%

                                                    Abundance N-15 = 0.37%

Explanation:

Data

Average atomic mass = 14.0067 amu

N-14 = 14.003074002

N-15 = 15.00010897

Abundance N-14 = ?   x

Abundance N-15 = ?   1 - x

Formula

Average atomic mass = (mass of N-14)x + (mass of N-15)(1 - x)

Substitution

14.0067 = 14.003074002x + 15.00010897(1 - x)

Solve for x

14.0067 = 14.003074002x + 15.00010897 - 15.00010897x

14.0067 - 15.00010897 = 14.003074002x - 15.00010897x

-0.9934 = -0.99703x

x = -0.9934 / -0.99703

x = 0.9963

Conclusion

Abundance N-14 = 0.9963 x 100 = 99.63 %

Abundance N-15 = 1 - 0.9963 = 0.0037 x 100 = 0.37 %

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