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How much electricity in terms of Faraday is required to produce 20 g of Ca from molten `CaCl_(2)` ? (Atomic mass of Ca =40 )

Text Solution

Verified by Experts

`CaCl_(2)hArrCa^(2+)+2Cl^(-)`
`underset("1 mole")(Ca^(2+))+underset(F)(2e)toCa`
40 g of Ca requires electricity =2F
20 g of Ca will require electricity
`=(2F)/(40)xx20`
=1F
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Knowledge Check

  • How much electricity in terms of Faraday is required to produce 100 g of Ca from molten CaCl_2 ?

    A
    1 F
    B
    2 F
    C
    3 F
    D
    5 F

  • How much electricity in terms of Faradays is required to produce 40.0 g of Al from molten Al_2O_3 ?

    A
    4.47 F
    B
    4.44 F
    C
    5.45 F
    D
    6.43 F

  • The number of Faradays (F) required to produce 20 g of calcium from molten CaCl_(2) (Atomic mass of Ca = 40 g mol^(-1) ) is

    A
    1
    B
    2
    C
    3
    D
    4

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    Explore conceptually related problems

    How much electricity in terms of Faraday is required to produce (i) 20.0 g of Ca from molten CaCl_(2) (ii) 40.0 g of Al from molten Al_(2)O_(3) .

    How much electricity in terms of Faraday is required to produce (i) 20.0 g of Ca from molten CaCl_2 ? (ii) 40.0 g of Al from molten Al_2O_3 ?

    How much electricity in term of Faraday is required to produce 40 gram of Al from Al_(2)O_(3) ? (Atomic mass of Al = 27 g/mol)

    How much electricity in terms in terms of Faraday is required to produce : (a) 20 g of Ca from molten CaCl_(2) (b ) 40 g of Al from molten Al_(2)O_(3) (Given : Molar mass of calcium and Aluminium are 40 g mol^(-1) and 27 g mol^(-1) respectively .)

    The number of Faradays(F) required to produce 20g of calcuim from molten CaCl_2 (Atomic massof Ca=40 gmol^-1 ) is:

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