Explain how the relative abundance of each Hydrogen isotope affects hydrogen's average atomic mass?

Question

Explain please thanks :)

Answer 1

The average mass is a weighted average of the isotope masses. If three isotopes of hydrogen have atomic masses 1,2, and 3, and the relative abundance of these are f1, f2, and f3 respectively (f being fractional proportion of each), then the average atomic mass is

1*f1+2*f2+3*f3

For example, if f1 = .9 (90% relative abundance), f2 = .08 (8% relative abundance) and f3 = .02 (2% relative abundance), then the weighted average would be

.9 + .16 + .06 = 1.12

A different set of relative abundances will give a different average atomic mass.

Answer 2

All factors see this result, no longer merely H. ok - you're able to desire to confirm the relative abundance of each and every isotope...when you consider that i won't be able to bear in mind, enable's merely placed some figures in for prepare. anticipate H1 has ninety 8% abundance, H2 has a million.5% and H3 0.5% which potential for each a hundred atoms of H, ninety 8 of them weigh a million amu, a million.5 of them weigh 2 amu and 0.5 of them weigh 3 amu so thats (ninety 8 x1) + (a million.5 x 2) + (0.5 x 3) = 102.5 amu for a hundred atoms 102.5/a hundred = a million.0.5 so as which may be the relative atomic mass. seek for the ideal suited %s and calculate it out.