Silver is a very precious metal and is used in jewellery. One million atoms of silver weight `1.79 xx 10^(-16)g`. calculate the atomic mass of silver.

Silver crsytallises in fcc lattice with all the atoms at the lattice points. The length of the edge of the unit cell as determined by X-ray diffraction studies is found 408.6 pm. The density of silver is 10.5 g cm^(-3) . Calculate the atomic mass of silver.

Silver crystallises in fcc lattice. If edge length of the cell is 4.07xx10^(-8) and density is 10.5 g cm^(-3) . Calculate the atomic mass of silver.

X-ray diffraction studies show that copper crystallises in a fcc unit cell with cell edge of 3.608 xx10^(-8) cm. In a separate experiment, copper is determined to have a density of 8.92 g//cm^(3) , calculate the atomic mass of copper.

An element with density 11.2 g cm^(-3) forms a fcc lattice with edge length of 4 xx 10^(-8) cm. Calculate the atomic mass of the element. (Given, N_(A)=6.022 xx 10^(23)"mol"^(-1) )

One gram of a mixture of KCl and KI dissolved in water and precipitated with silver nitrate 1.618g of silver halides are obtained calculate the percentage composition of mixture.

Silver is electrolytically deposited on a metallic vessel of total surface area 900 c m^(2) by passing a current of 0.5A for 2h. Calculate the thickness of silver deposited . Given, density of silver =10.5 g c m^(-1) . Atomic mass of silver = 108u, F = 96500 C "mol"^(-1)

Copper crystallises with face centred cubic unit cell. If the radius of copper atom is 127.8 pm, calculate the density of copper metal. (Atomic mass of Cu= 63.55 u and Avogadro's number, N_(A)=6.02xx10^(23)"mol"^(-1) )

Two elements A and B form compounds having molecular formula AB_(2) and AB_(4) When dissolved in 20 g of benzene, 1 g of AB_(2) lowers the freezing point by 2.3 K, whereas 1.0 g of AB_(4) lowers it by 1.3 K. The molar depression constant for benzene is 5.1 K kg mol^-1 . Calculate the atomic mass of A and B.