IsotopeRelative abundance (%)Atomic mass (u)^ | vedclass

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(A) The average atomic mass of carbon is calculated as follows:Average atomic mass of $C = (0.988 	imes 12) + (0.0118 	imes 13.1) + (0.0002 	imes 1

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$16.0452$

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(A) The average atomic mass of carbon is calculated as follows:Average atomic mass of $C = (0.988 	imes 12) + (0.0118 	imes 13.1) + (0.0002 	imes 14.1)$$= 11.856 + 0.15458 + 0.00282 = 12.0134 \ u$The molecular mass of $CH_4$ is given by the sum of the average atomic mass of carbon and $4$ times the atomic mass of hydrogen:Molecular mass of $CH_4 = 12.0134 + (4 	imes 1.008)$$= 12.0134 + 4.032 = 16.0454 \ u$Rounding to the nearest provided option,the correct value is $16.0452 \ u$.

Isotope	Relative abundance $(\%)$	Atomic mass $(u)$
$^{12}C$	$98.8$	$12$
$^{13}C$	$1.18$	$13.1$
$^{14}C$	$0.02$	$14.1$

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IsotopeRelative abundance $(\%)$Atomic mass $(u)$$^{12}C$$98.8$$12$$^{13}C$$1.18$$13.1$$^{14}C$$0.02$$14.1$From the above data,what is the average molecular mass of $CH_4$ containing all isotopes of carbon,assuming hydrogen is only $^{1}_{1}H$? (Given that atomic mass of hydrogen $= 1.008 \ u$)