IsotopeRelative Abudance(%)Atomic Mass(amu)12C98.8921213C1.10813.00335

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\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

Options:

A . 13 u

B . 12.011 u

C . 12.001 u

D . 12.0011 u

Answer: Option B
:
B
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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