Relative abundance of isotopes of carbon are as follows- - - -Isotopes nbsp- nbsp- - nbsp- Relative abundance nbsp- nbsp- - nbsp- Atomic Mass nbsp- - - -C-12 - nbsp- 98-892 - nbsp- 12 - - -C-13 - nbsp- 1-108 - nbsp- 13-00335 - - -C-14 - nbsp- 2-10-10 - nbsp- 14-00317 - - The average atomic mass of carbon will be-16-0056 u-12-001 u-15-001 u-10-001 u-

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Atomic Mass

Relative abun...

Question

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:-

16.0056 u

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12.001 u

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15.001 u

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10.001 u

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Solution

The correct option is B 12.001 u
The average atomic mass of an element is the sum of the masses of its isotopes, each multiplied by its natural abundance.

Atomic Weight =(% abundance isotope 1)×mass of isotope 1 +(% abundance isotope 2)×mass of isotope 2 +(% abundance isotope 3)×mass of isotope 3 /100
Hence, average atomoc weight of C =
$\frac{(98.892 \times 12) + (1.108 \times 13.00335) + (2 \times 10^{- 10} \times 14.00317)}{100}$

= 12.001 u

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

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 2×10−10 14.00317 The average atomic mass of carbon will be:-

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:-