In nature,carbon exists as a mixture of C^{12 | vedclass

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(B) Let the percentage abundance of $C^{12}$ be $x\%$ and that of $C^{13}$ be $(100-x)\%$.The average atomic mass is given by the formula:$	ext{Avera

Vedclass · Accepted Answer

$98.9$

Vedclass · Answer

(B) Let the percentage abundance of $C^{12}$ be $x\%$ and that of $C^{13}$ be $(100-x)\%$.The average atomic mass is given by the formula:$	ext{Average Atomic Mass} = \frac{(x 	imes 12) + ((100 - x) 	imes 13)}{100}$Substituting the given values:$12.011 = \frac{12x + 1300 - 13x}{100}$$12.011 = \frac{1300 - x}{100}$$1201.1 = 1300 - x$$x = 1300 - 1201.1$$x = 98.9\%$Therefore,the abundance of $C^{12}$ is $98.9\%$.

In nature,carbon exists as a mixture of $C^{12}$ and $C^{13}$. The average atomic mass of carbon is $12.011$. What is the percentage abundance of $C^{12}$ in nature?

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