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Chemistry · Some Basic Concepts of Chemistry
हिन्दीIf the average atomic mass of carbon is calculated using the isotopes \( ^{12}\text{C} \) (98.892%, 12 u), \( ^{13}\text{C} \) (1.108%, 13.00335 u), and \( ^{14}\text{C} \) (\( 2 \times 10^{-10}\%, 14.00317 \text{ u} \)), what is the resulting average atomic mass of carbon?
Correct answer · Option 4
\( 12.011 \text{ u} \)
Explanation
Average atomic mass = \( \sum (\text{fractional abundance} \times \text{isotopic mass}) = 12.011 \text{ u} \).
