Neon occurs as two isotopes of mass numbers 20 and 22. Its relative atomic mass is 20.2. What is the percentage of ²⁰Ne in naturally occurring neon?

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Solution

The correct option is D
90

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Q. Neon has two isotopes,

^{20} N e

and

^{22} N e

. If atomic weight of Neon is 20.2, then the ratio of the relative abundances of the isotopes is:

Given that the percentage abundance of the isotope $_{10}^{20} N e$ , is 90% and that of the isotope $_{10}^{22} N e$ is 10%, calculate the average atomic mass of neon.

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Q. Atomic weight of Ne is 20.2. Ne is mixture of

N e^{20}

and

N e^{22}

, relative abundance of heavier isotopes is:

The three stable isotopes of neon: and have respective abundances of 90.51%, 0.27% and 9.22%. The atomic masses of the three isotopes are 19.99 u, 20.99 u and 21.99 u, respectively. Obtain the average atomic mass of neon.

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Neon occurs as two isotopes of mass numbers 20 and 22. Its relative atomic mass is 20.2. What is the percentage of 20Ne in naturally occurring neon?

The correct option is D 90

Neon occurs as two isotopes of mass numbers 20 and 22. Its relative atomic mass is 20.2. What is the percentage of ²⁰Ne in naturally occurring neon?

The correct option is D
90