If two naturally occurring isotopes of an element are −X15 and −X11, what is the % age composition of each isotope of X occurring respectively, if the average atomic weight accounts to 14?
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Let the percentage of boron isotope with atomic weights 10.01 be x% and that of atomic weight 11.01 be (100-x)%. Average atomic mass of boron is 10.81.
Average atomic mass =
100
Atomic weight of first isotope×x+atomic weight of second isotope×(100−x)
10.81=
100
10.01x+11.01×(100−x)
x=20
(100−x)=80
Hence, natural abundance of isotope with atomic weight 10.01 is 20%
natural abundance of isotope with atomic weight 11.01 is 80%
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