In a NaCI type crystal distance between Na^+and Cl^-ion is 2.814 A^{†extdegree\overline{}} and the density of solid is 2.167 g cm^{-^3} then find out the value of Avogadroconstant.

Q. In a NaCl type crystal distance between $N{a}^{+}$ and $C{l}^{-}$ ion is $2.814\mathring{A}$ and the density of solid is $2.167gm/c{m}^3$ then find out the value of Avogadro constant.

Q. Formula mass of NaCl is $58.45$ g mol${}^{-1}$ and density of its pure form is $2.167$ g cm${}^{-3}$. The average distance between adjacent sodium and chloride ions in the crystal is $2.814\times {10}^{-8}$ cm. Calculate Avogadro's constant.

Q. Calculate the value of Avagadro's number if the density of $NaCl$ is $2.165$ g cm${}^{-3}$ and distance between $N{a}^{+}$ and $C{l}^{-}$ ions in $NaCl$ crystal is $281$ pm.

Q. The distance between $N{a}^{+}$ and $C{l}^{-}$ ions in $NaCl$ with a density $3.165$ g $c{m}^{-3}$ is:

Q. What is the distance between ${Na}^{+}$ and ${Cl}^{-}$ ions in $NaCl$ crystal if its density is $2.165g{cm}^{-3}$ .[Atomic mass of $Na-23u,Cl=35.5u$, Avogadro,s Number=$6.023\times {10}^{23}$]