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A solution of CuSO(4) is electroysed for...

A solution of `CuSO_(4)` is electroysed for 10 minutes with a current of 1.5 amperes. What is the mass of copper deposited at the cathode ?
(Molar mass of `Cu=63.5 g//mol)`

Text Solution

Verified by Experts

`I=1.5" Ampere"`
`"Time "=10xx60s=600s`
`Q=Ixxt`
`=1.5xx600=900C`
`Cu^(2+)+2e^(-)rarrCu(s)`
2F amount of electricity deposit copper = 63.5 g
`"900 C amount of electricity deposit copper"=(63.5xx900)/(2xx96500)`
`=0.296g`
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A solution of CuSO_(4) is electrolysed for 10 minutes with a current of 1.5 amperes. What is the mass of copper deposited at the cathode? (Molar mass of Cu=63.5 g mol^(-1) )

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Knowledge Check

  • A solution of CuSO_(4) is electrolsed for 10 minutes with a current of 1.5 amperes. What is the mass of copper deposited at the cathode ? (Molar mass of Cu=63.5 g//mol)

    A
    0.492 g
    B
    0.325 g
    C
    0.873 g
    D
    0.296 g

  • Two faradays of electricity are passed through a solution of CuSO_(4) .The mass of copper deposited at the cathode is (atomic mass of Cu=63.5 g)

    A
    2 g
    B
    127 g
    C
    0 g
    D
    63.5 g

  • Two Faraday of electricity is passed through a solution of CuSO_(4) . The mass of copper deposited at the cathode is : (at mass of Cu = 63.5 amu)

    A
    2 g
    B
    127 g
    C
    0 g
    D
    63.5 g

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    Two faradays of electricity are passed through a solution of CuSO_(4) . The mass of copper deposited at the cathode (at. Mass of Cu=63.5 amu)

    Two faraday of electricity is passed through a solution of CuSO_(4) . The mass of copper deposited at the cathode is: (at mass of Cu = 63.5 amu)

    Two faraday of electricity is passed through a solution of CuSO_(4) . The mass of copper deposited at the cathode is (at. Ass of Cu=63.5 amu)

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