Calculate the reported average elemental atomic mass of O if the naturally occurring isomers are 16 O -17 O- and 18 O- Their masses and abundance areas follows- array - c - c - c - hline-16 O - 15-995 - 99-761 - llhhine -17 O - 16-999 - 0-041 - -18 O - 17-999 - 0-21 - lllhline e n d a r r a y A- 16-02B- 15-98C- 15-52D- 16-3

The correct option is B 15.98The average elemental atomic mass of Mg will be nbsp; = 15.995 × 0.997+16.999 × 0.0004+17.999 × 0.002 = 15.98 amu nbsp; ...

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Standard XII

Chemistry

Mole Concept

Calculate the...

Question

Calculate the reported average elemental atomic mass of $O$ if the naturally occurring isomers are $^{16} O,^{17} O, a n d^{18} O$ . Their masses and abundance are as follows:
$\begin{matrix} Isotope & Atomic Mass & Isotopic Abudance^{16} O & 15.995 & 99.76 %^{17} O & 16.999 & 0.04 %^{18} O & 17.999 & 0.2 % \end{matrix}$

16.02

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15.98

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15.52

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16.3

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Solution

The correct option is B 15.98
The average elemental atomic mass of $M g$ will be
$= 15.995 \times 0.997 + 16.999 \times 0.0004 + 17.999 \times 0.002$
$= 15.98$ amu

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Calculate the reported average elemental atomic mass of O if the naturally occurring isomers are 16O, 17O, and 18O. Their masses and abundance are as follows: IsotopeAtomic MassIsotopic Abudance16O15.99599.76%17O16.9990.04%18O17.9990.2%

The correct option is B 15.98The average elemental atomic mass of Mg will be =15.995×0.997+16.999×0.0004+17.999×0.002 =15.98 amu

The correct option is B 15.98
The average elemental atomic mass of $M g$ will be
$= 15.995 \times 0.997 + 16.999 \times 0.0004 + 17.999 \times 0.002$
$= 15.98$ amu