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Copper crystallises with face-centred cu...

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 g/mol and Avogadro's number `N_(A) = 6.02 xx 10^(23) mol^(-1)`)

Text Solution

Verified by Experts

fcc `rarr` 4 atoms = Z
r = 127.8 pm
`r = (a)/(2 sqrt(2))`
`therefore" "a = 127.8 xx 2 sqrt(2)`
= 361.47 pm
`d = (Z xx M)/(a^(3) xx N_(A))`
`d = (4 xx 63.55 g mol -1 )/((361.47 xx 10^(-12)m)^(3) xx 6.02 xx 10^(23) mol^(-1))`
= 8.9 `gm^(-3)`
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