Question

Nitrogen occurs in nature in the form of 2 isotopes with atomic mass 14 & 15 respectively. If average atomic mass of nitrogen is 14.0067,what is the % abundance of two isotopes

Answer 1

Let x be the percent abundance of N - 14 isotopes. Then there's the bulk of percent abundance $\frac{x+14+(100-x)x15}{100}$

Step-by-step-explanation:

After solving the equation, we get,

$\frac{x+14+(100-x)x15}{100}$=14.0067

−x=1400.67 −1500=−99.33

x=99.33

Thus % abundance of N-14 isotope = 99.33%

% abundance of N-15 isotope = 100 - 99.33 = 0.67%

Hence, the percent abundance of the two isotopes is 99.33 % and 0.67% respectively.

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