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(D) Step $1$: The mass of a single unit cell is given by the product of density $(\rho)$ and volume of the unit cell $(V_{uc})$.Mass of one unit cell

Vedclass · Accepted Answer

$4.0 	imes 10^{21}$

Vedclass · Answer

(D) Step $1$: The mass of a single unit cell is given by the product of density $(ho)$ and volume of the unit cell $(V_{uc})$.Mass of one unit cell = $ho 	imes V_{uc} = 2.5 	imes 10^{-22} 	ext{ g}$.Step $2$: The number of unit cells in a given mass $(m)$ is calculated using the formula: $	ext{Number of unit cells} = \frac{	ext{Total mass}}{	ext{Mass of one unit cell}}$.Step $3$: Substitute the given values: $	ext{Number of unit cells} = \frac{1 	ext{ g}}{2.5 	imes 10^{-22} 	ext{ g}} = \frac{1}{2.5} 	imes 10^{22} = 0.4 	imes 10^{22} = 4.0 	imes 10^{21}$.Thus, the correct option is $D$.

Calculate the number of unit cells present in $1 \text{ g}$ of a metal if the product of the density of the metal and the volume of the unit cell is $2.5 \times 10^{-22} \text{ g}$.

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