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zhenek [66]
3 years ago
13

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. %
Chemistry
1 answer:
Ymorist [56]3 years ago
6 0

Answer:

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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Answer:

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Explanation:

The number of molecules is present in any mole of an element or compound are the same. To find the molecules you need to multiply the number of the moles of the compound by Avogadro's number:

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