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Standard XII

Chemistry

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Ice crystalli...

Question

Ice crystallizes in a hexagonal lattice. At low temperature, at which the structure was determined, the lattice constants were $a = 4.53 ˚ A$ and $b = 7.60 ˚ A$ (see figure). How many molecules of water are contained in a given unit cell? [Density of ice is $0.92$ g cm $^{- 3}$ .]

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Solution

The correct option is C $4$
As we know, density $= \frac{n M}{V N_{o}}$ , where n is the number of atoms per unit cell.
Density $= 0.92 = \frac{n \times 18}{(a^{2} b) \times (6 \times 10^{23})}$ $⟹ n = 4$
So, one unit of this structure contains $4$ molecules of water.

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Similar questions

Q. Ice crystallizes in a hexagonal lattice. At the low temperature at which the structure was determined, the lattice constants were

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Ice crystallizes in a hexagonal lattice. At low temperature, at which the structure was determined, the lattice constants were a=4.53 ˚A and b=7.60 ˚A (see figure). How many molecules of water are contained in a given unit cell? [Density of ice is 0.92 g cm−3.]

The correct option is C 4As we know, density =nMVNo, where n is the number of atoms per unit cell.Density =0.92=n×18(a2b)×(6×1023) ⟹n=4So, one unit of this structure contains 4 molecules of water.

Ice crystallizes in a hexagonal lattice. At low temperature, at which the structure was determined, the lattice constants were $a = 4.53 ˚ A$ and $b = 7.60 ˚ A$ (see figure). How many molecules of water are contained in a given unit cell? [Density of ice is $0.92$ g cm $^{- 3}$ .]

The correct option is C $4$
As we know, density $= \frac{n M}{V N_{o}}$ , where n is the number of atoms per unit cell.
Density $= 0.92 = \frac{n \times 18}{(a^{2} b) \times (6 \times 10^{23})}$ $⟹ n = 4$
So, one unit of this structure contains $4$ molecules of water.