Question

it nature N have two isotopes N-14 and N-15 with atomic masses 14and 15 respectively with abundance in nature 99.63% and 0.37% calculate Average atomic mass ​

Answer 1

Explanation:

$14 \times 99.63 \div 100 + 15 \times 0.37 \div 100$

$13.9482 + 0.0555$

$= 14.0037\%$

How did I find the a.m.u?

Average atomic mass is the average value of atomic mass of isotopes.

to calculate a.m.u, we need

Mass of isotopes mentioned

Natural abundance of isotopes

we multiply them and divide them with 100 to find the percentage.

hope this helps..