X=5Å Y=8Å Molar mass of solid =259.8 g mol^(-1) A solid crystallises in hexagonal lattice as shown in above figure. Density of the solid is 5 g/ml…

Question

X=5Å Y=8Å Molar mass of solid =259.8 g mol^(-1) A solid crystallises in hexagonal lattice as shown in above figure. Density of the solid is 5 g/ml . How many molecules are their in the given unit cell? (Avagadro's number =6.023×10^23 )

MARKS Content Team · Accepted Answer

Correct answer: (A) 2. Volume of unit cell = Area of base × height =X^2sin⁡60°×Y =5×10^(-8)2×0.866×8×10^(-8) =1.732×10^(-22)cm^3 Number of molecules in the unit cell =(Volume×Density)/(Molar mass)×6.023×10^23 =(1.732×10^(-22)×5)/259.8×6.023×10^23≈2 .

$X = 5 Å$
$Y = 8 Å$
Molar mass of solid $= 259.8 g mo l^{- 1}$

A solid crystallises in hexagonal lattice as shown in above figure. Density of the solid is $5 g/ml$ . How many molecules are their in the given unit cell?
(Avagadro's number $= 6.023 \times 1 0^{23}$ )

Solution

More Solid State Questions

X=5Å Y=8Å Molar mass of solid =259.8 g mol-1 A solid crystallises in hexagonal lattice as shown in above figure. Density of the solid is 5 g/ml . How many molecules are their in the given unit cell? (Avagadro's number =6.023×1023 )

Solution

More Solid State Questions

$X = 5 Å$
$Y = 8 Å$
Molar mass of solid $= 259.8 g mo l^{- 1}$

A solid crystallises in hexagonal lattice as shown in above figure. Density of the solid is $5 g/ml$ . How many molecules are their in the given unit cell?
(Avagadro's number $= 6.023 \times 1 0^{23}$ )