Nitrogen is made up of two isotopes, N-14 and N-15. Given nitrogen's atomic weight of 13.007, what is the percent abundance of each isotope?
2007-08-22 17:37:46 · 4 answers · asked by d 1 in Science & Mathematics ➔ Chemistry
Let x = the relative fraction of N-14
Let (1-x) = the relative fraction of N-15
So:
14x + (1-x)15 = 14.007
14x + 15 - 15x =14.007
-x + 15 =14.007
15 = 14.007 + x
x=0.993
% N-14 = 99.3
% N-15 = 0.7
Check: 0.993 x 14 + 0.007 x 15 = 14.007
2007-08-22 18:15:00 · answer #1 · answered by Flying Dragon 7 · 2⤊ 0⤋
Isotopes Of Nitrogen
2016-10-15 02:45:48 · answer #2 · answered by clausel 4 · 0⤊ 0⤋
14 (X ) + 15 (100-X) = 14.007 (100) that's your equation solve for X and 100-X X ===> amount % nitrogen 14 100-X ====> amount % nitrogen 15 EDIT ====== Since 14.003 amu and 15.0001 amu are not given in the problem, I still think that you should use 14 and 15 in the equation. The average atomic mass given is 14.007, not 14.01. ( Not that, it will affect the end result much..) When you are given certain data, you are expected to solve the problem with that given data.
2016-03-13 00:15:40 · answer #3 · answered by Anonymous · 0⤊ 0⤋
Flying dragon has given u the correct method
2007-08-22 22:28:22 · answer #4 · answered by mythili 2 · 0⤊ 0⤋