The relative atomic mass of an element A is 16.2. There are two isotopes 16 and 18 of the element. Determine the adequacy in nature of the isotopes.
Answers
Answer:
Aɴsᴡᴇʀ:-
Data:-
Relative atomic mass=16.2
✯ Atomic mass of 8^16
A=16
✯ Atomic mass of 8^18
A=18
Formula:-
Let percentage of Isotope 8^16
A be ⟶x
∴ Percentage of Isotope
818
A⟶(100−x)
Relative atomic weight=
[Atomic weight of 8^16 A× abundance+ Atomic weight of 8^18 A× abundance]/100
∴16.2= 100
16×x+18×(100−x)
= 100
16x×1800−18x
⇒16.2×100=1800−2x
⇒1620=1800−2x
⇒2x=1800−1620
⇒2x=180
∴x=90
100−x=10
✯ Percentage of 8^16
A is 90%.
✯ Percentage of 8^18
A is 10% .
Answer:
Answer
Data:-
Relative atomic mass=16.2
Atomic mass of
8
16
A=16
Atomic mass of
8
18
A=18
Formula:-
Let percentage of Isotope
8
16
A be ⟶x
∴ Percentage of Isotope
8
18
A⟶(100−x)
Relative atomic weight=[Atomicweightof
8
16
A×abundance+Atomicweightof
8
18
A×abundance]/100
∴16.2=
100
16×x+18×(100−x)
=
100
16x×1800−18x
⇒16.2×100=1800−2x
⇒1620=1800−2x
⇒2x=1800−1620
⇒2x=180
∴x=90
100−x=10
Percentage of
8
16
A is 90%
Percentage of
8
18
A is 10% .
Explanation:
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