(C) The molar mass of $NaCl$ is $58.5 \, g/mol$. Given mass $W = 58.5 \, g$. Number of moles $n = \frac{W}{M} = \frac{58.5}{58.5} = 1 \, mol$. Total n

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(C) The molar mass of $NaCl$ is $58.5 \, g/mol$. Given mass $W = 58.5 \, g$. Number of moles $n = \frac{W}{M} = \frac{58.5}{58.5} = 1 \, mol$. Total number of $NaCl$ formula units $= n \times N_A = 1 \times 6 \times 10^{23} = 6 \times 10^{23}$. In an $fcc$ structure,the number of formula units per unit cell $(Z)$ is $4$. Number of unit cells $= \frac{\text{Total formula units}}{Z} = \frac{6 \times 10^{23}}{4} = 1.5 \times 10^{23}$.

Class 12 Chemistry Solid State Mathematical analysis of cubic system and Bragg’s equation

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Calculate the number of unit cells in $58.5 \, g$ of $NaCl$ crystallizing in an $fcc$ structure. $(NaCl = 58.5 \, g/mol)$

A
$6 \times 10^{20}$
B
$3 \times 10^{22}$
C
$1.5 \times 10^{23}$
D
$0.5 \times 10^{24}$

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Mathematical analysis of cubic system and Bragg’s equation

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Calculate the number of unit cells in $58.5 \, g$ of $NaCl$ crystallizing in an $fcc$ structure. $(NaCl = 58.5 \, g/mol)$

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In a $bcc$ lattice having the edge length of $200 \ pm$, the cation has the radius of $70 \ pm$. The radius ratio of $\frac{r^{+}}{r^{-}}$ is (Given, $\sqrt{2}=1.4, \sqrt{3}=1.7$ and $\sqrt{6}=2.4$ )

Copper crystallises into a $fcc$ lattice with edge length $3.61 \times 10^{-8} \, cm$. Show that the calculated density is in agreement with its measured value of $8.92 \, g \, cm^{-3}$.

$A$ binary compound $(A^{+} B^{-})$ has a rock salt structure. If the edge length is $400 \, pm$ and the radius of the cation $(A^{+})$ is $75 \, pm$, what is the radius of the anion $(B^{-})$ in $pm$?

Calculate the number of unit cells in $1 \, g$ of $NaCl$ crystal,which crystallizes in an $fcc$ structure. (Molar mass of $NaCl = 58.5 \, g/mol$)

The number of atoms in $100 \ g$ of an $fcc$ crystal with density $d = 10 \ g/cm^3$ and cell edge equal to $100 \ pm$ is equal to

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