The density of ice is 0.921 g cm^(3) calculate the mass of cubic block of ice which is 76 mm on each side.

Density of a unit cell is respresented as rho = (" Effective no. of atoms (s)" xx "Mass of a unit cell ")/("Volume of a unit cell ")=(Z.M)/(N_(A).a^(3)) where , mass of unit cell =mass of effectuive no . of atoms(s) or ion (s). M= At . mass// formula N_(A) = Avogadro' s no . rArr 6.0323 xx 10^(23) a= edge lemght of unit cell The density of KBr is 2.75 g //cm^(-3) . The length of the edge of the unit cell is 645 pm .To which type of cubic crystal , KBr belongs ?

An element E crystallizes in boyd centred cubic structure. If the edge lengh of the cell is 1.469xx10^-10m and the denstiy is 19.3 g cm^-3 , calculate the atomic mass of this element. Also calculate the radius of an atom of the element.

Niobium crystallizes in a body centred cubic structure. If density is 8.55 "gcm"^(-3) , calculate atomic radius of niobium, given that its atomic mass is 92.9mu .

Hundred gram of Al(HNO_3)_3 (molar mass 213 gmol^-1 ) is dissolved in 1 L of water at 20^@C . The density of water at this temperature is 0.9983 gcm^-3 and the density of resulting solution is 0.9990 gcm^-3 . Calculate the molarity and molality of this solution.

Niobium crystallises in body-centred cubic structure. If density is 8.55g cm^(-3) , calcuate atomic radius of niobium using its atomic mass 93 u.

Caesium chlorde cystallised as cubic lattices and has a density of 4.0 gcm^-3 . Calculate the length of the edge of the unit cell of caesium chloride.( Molar mass of CsCl=168.5 gmol^-1 ).

The density of chromium metal is 7.2"g cm"^(-3) . If the unit cell is cubic with edge length of 289 pm, determine the type of unit cell. Atomic mass of Cr = 52 a.m.u., N_(0)=6.02xx10^(23)"mol"^(-1) .

The density of KBr is 2.75"gm cm"^(-3) . The edge length of unit cell is 654 pm. Predict the type of cubic lattice to which unit cell of KBr belongs. (N_(0)=6xx023xx10^(23)"mol"^(-1)) . Atomic mass of K = 39, Br = 80.