Which of the following has the largest number | vedclass

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(D) To find the number of atoms, we use the formula: $	ext{Number of atoms} = \frac{	ext{mass}}{	ext{molar mass}} 	imes 	ext{atomicity} 	imes N_

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$1 \ g$ of $Mg$

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(D) To find the number of atoms, we use the formula: $	ext{Number of atoms} = \frac{	ext{mass}}{	ext{molar mass}} 	imes 	ext{atomicity} 	imes N_{A}$.For $A$: $1 \ g$ of $Ag$ (atomic mass = $108 \ g/mol$): $	ext{Atoms} = \frac{1}{108} 	imes 1 	imes N_{A} \approx 0.0092 \ N_{A}$.For $B$: $1 \ g$ of $Fe$ (atomic mass = $56 \ g/mol$): $	ext{Atoms} = \frac{1}{56} 	imes 1 	imes N_{A} \approx 0.0178 \ N_{A}$.For $C$: $1 \ g$ of $Cl_{2}$ (molar mass = $71 \ g/mol$): $	ext{Atoms} = \frac{1}{71} 	imes 2 	imes N_{A} \approx 0.0281 \ N_{A}$.For $D$: $1 \ g$ of $Mg$ (atomic mass = $24 \ g/mol$): $	ext{Atoms} = \frac{1}{24} 	imes 1 	imes N_{A} \approx 0.0416 \ N_{A}$.Comparing the values, $1 \ g$ of $Mg$ has the largest number of atoms.

Which of the following has the largest number of atoms?

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