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Vapour density of a metal chloride is 54...

Vapour density of a metal chloride is 54 . Metal content of the compound is 34.32 % . Calculate the atomic weight of the metal .

Text Solution

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The metal chloride contains 34.32 % metal .
`therefore` The metal chloride contains (100-34.32) = 65.68% chlorine . Hence , the equivalent weight (E) of the metal = `(34.32)/(65.68) xx 35.5 = 18.85`
Molecular weight of the metal chloride = `54 xx 2 = 108`
Let the molecular formula of the metal chloride be `MCl_(v)` [where , V = valency of the metal]
`therefore` Molecular weight of `MCl_(V) = A + 35.5 V` [ where A = atomic weight of the metal ]
We know , `A = E xx V ` or `A = 18.55 xx V`
Hence `(18.55 xx V) + (35.5 xx V) = 108` or `V = (108)/(54.05) = 2`
`therefore` Atomic weight of the metal = `18. 55 xx 2 = 37.1`
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Knowledge Check

  • The chloride of a metal contains 54.4% of chlorine. The vapour density of the chloride is 130.56. Find the atomic mass of the metal

    A
    24
    B
    119
    C
    86
    D
    56

  • The chloride of a metal contains 71% chlorine by weight and the vapour density of it is 50. The atomic weight of the metal will be

    A
    29
    B
    58
    C
    35.5
    D
    71