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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 the unit is redefined as $1/6$ of the mass of a c

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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 the unit is redefined as $1/6$ of the mass of a carbon-$12$ atom, the new unit $(amu')$ is $2$ times the original unit $(amu' = 2 	imes amu)$. The molar mass of a substance is defined as the mass of $N_A$ particles, where $N_A$ is the Avogadro constant. By definition, $1 	ext{ mole}$ of carbon-$12$ has a mass of $12 	ext{ g}$. If the mass of one unit is doubled, the number of units required to make $12 	ext{ g}$ of carbon-$12$ will be halved. Thus, the new Avogadro constant $N_A'$ becomes $N_A/2$. The mass of one mole of a substance is given by $M = (	ext{mass of one particle}) 	imes N_A$. Since the mass of one particle is expressed in the new units, it becomes $m' = m/2$. Therefore, the new molar mass $M' = m' 	imes N_A' = (m/2) 	imes (N_A/2) = M/4$. However, in standard chemistry problems of this type, if the reference standard for the mole is fixed at $12 	ext{ g}$ of carbon, the mass of one mole of any substance remains $12 	ext{ g/mol}$ relative to the new scale, but the absolute mass in grams changes. Given the options, the mass of one mole (as a numerical value in the new scale) remains unchanged.

If we consider that $1/6$ of the mass of a carbon-$12$ 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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