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An element occurs in bcc structure with cell edge 288 pm. Its density is 7.2 g cm^(-3). Calculate the atomic mass of the element.

Answer»


Solution :Z = 2 for bcc structure , a=288 PM, d = 7.2 g `CM^(-3)`, `N_A =6.023 xx 10^(23) MOL^(-1)`
`M= (N_A xx d xx a^3)/(Z)=(6.023 xx 10^(23) xx 7.2 xx (288)^3 xx 10^(-30))/(2) = 51.79 g mol^(-1)`


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