To find the percent abundance of each isotope of nitrogen, we need to determine the ratio of the masses of the isotopes and use it to calculate the percentage.
Let X be the percent abundance of N-14 and 100-X be the percent abundance of N-15.
The atomic weight of nitrogen can be expressed as:
(14 * X/100) + (15 * (100-X)/100) = 14007.
Expanding the equation:
(14X/100) + (1500 - 15X)/100 = 14007.
Multiplying both sides by 100 to eliminate the denominators:
14X + 1500 - 15X = 1400700.
Subtracting 1500 from both sides:
-X = 1400700 - 1500.
Simplifying:
-X = 1400200.
Dividing both sides by -1:
X = -1400200.
Therefore, the percent abundance of N-14 is -1400200 and the percent abundance of N-15 is 100 - (-1400200) = 100 + 1400200 = 1400300.
However, since negative percent abundance is not possible, it seems like there might be an error in the given information or calculation. Please make sure to double-check the values provided.
Nitrogen is made up of two isotopes, N-14 and N-15. Given nitrogen's atomic weight of 14007, what is the percent abudence of each isotope
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