Begin array - c - c - c WhineIsotope - Relative Abudance1- - Atomic Massamu-lhline-13 C - 1-108 - 13-00335 Illhline-14 C - 2 10-10 - 14-00317 INhline end array From the data given in the table- calculate the average atomic mass of CA- 13 uB- 12-001 uC- 12-011 uD- 12-0011 u

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Standard XII

Chemistry

Percentage Composition

begin array |...

Question

$\begin{matrix} I s o t o p e & R e l a t i v e A b u d a n c e (%) & A t o m i c M a s s (a m u)^{12} C & 98.892 & 12^{13} C & 1.108 & 13.00335^{14} C & 2 \times 10^{- 10} & 14.00317 \end{matrix}$

From the data given in the table, calculate the average atomic mass of C

13 u

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12.011 u

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12.001 u

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12.0011 u

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Solution

The correct option is B 12.011 u
Average atomic mass is the weighted average of atomic mass of all the isotopes.
Contribution by each isotope = (Relative abundance) (Atomic mass)
Contribution by
$_{6}^{12} C$ = (0.98892)(12)/100 = 11.86704

$_{6}^{13} C$ = (0.01108)(13.00335)/100 = 0.14407712

$_{6}^{14} C$ = (2 $\times$ $10^{- 10}$ )(14.003170/100 = 28.00634 $\times$ $10^{- 12}$

$∴$ Average atomic mass = sum of all contribution = 12.011 u

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Similar questions

$\begin{matrix} Isotope & Relative Abudance (%) & Atomic Mass(amu)^{12} C & 98.892 & 12^{13} C & 1.108 & 13.00335^{14} C & 2 \times 10^{- 10} & 14.00317 \end{matrix}$

From the data given in the table, calculate the average atomic mass of C

\begin{matrix} I s o t o p e & R e l a t i v e A b u d a n c e (%) & A t o m i c M a s s (a m u)^{12} C & 98.892 & 12^{13} C & 1.108 & 13.00335^{14} C & 2 \times 10^{- 10} & 14.00317 \end{matrix}

From the data given in the table, calculate the average atomic mass of C.

Relative abundance of isotopes of carbon are as follows:-

Isotopes	Relative abundance	Atomic Mass
C-12	$98.892$	12
C-13	$1.108$	13.00335
C-14	$2 \times 10^{- 10}$	14.00317

The average atomic mass of carbon will be:-

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IsotopeRelative Abudance(%)Atomic Mass(amu)12C98.8921213C1.10813.0033514C2×10−1014.00317 From the data given in the table, calculate the average atomic mass of C

$\begin{matrix} I s o t o p e & R e l a t i v e A b u d a n c e (%) & A t o m i c M a s s (a m u)^{12} C & 98.892 & 12^{13} C & 1.108 & 13.00335^{14} C & 2 \times 10^{- 10} & 14.00317 \end{matrix}$

From the data given in the table, calculate the average atomic mass of C