If we consider that 1/6 of the mass of a carb | vedclass

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(C) The relative atomic mass unit $(amu)$ is defined as $1/12$ of the mass of a carbon-$12$ atom. If we redefine the unit as $1/6$ of the mass of a ca

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Remain unchanged

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(C) The relative atomic mass unit $(amu)$ is defined as $1/12$ of the mass of a carbon-$12$ atom. If we redefine the unit as $1/6$ of the mass of a carbon-$12$ atom,the new unit $(amu')$ becomes $2$ times the original unit $(amu' = 2 	imes amu)$. Since the mass of one mole of a substance is defined as the mass of $N_A$ atoms (where $N_A$ is the Avogadro constant),and the definition of the mole is linked to the mass of $12 \, g$ of carbon-$12$,changing the reference unit changes the Avogadro number. Specifically,if the unit mass is doubled,the number of particles required to make up the same macroscopic mass is halved $(N_A' = N_A/2)$. Therefore,the mass of one mole of a substance,which is the product of the number of particles and the mass per particle,remains unchanged because the increase in the mass of the unit is exactly compensated by the decrease in the Avogadro number.

Isotope	$\%$ Natural abundance	Molar mass
$^1H$	$99.985$	$1$
$^2H$	$0.015$	$2$

If we consider that $1/6$ of the mass of a carbon atom,in place of $1/12$,is taken to be the relative atomic mass unit,the mass of one mole of a substance will

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Isotope $\%$ Natural abundance Molar mass

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