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A current of 1.50 A was passed through a...

A current of 1.50 A was passed through an electrolytic cell containing `AgNO_3` solution with inert electrodes. The weight of silver deposited was 1.50 g. How long did the current flow ? [Molar mass of `Ag = 108 g mol^(-1)`?, 1 F = `96500 C mol^(-1)`]

Text Solution

Verified by Experts

Quantity of charge required to deposit 108 g Ag = 96500 C
Quantity of charge required to deposit 1.5 g Ag `=(96500)/108 xx 1.5 = 1340.28 C`
Time taken `=Q/l = (1340.28)/1.50 = 893.5s`
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A current of 1.50 A was passed through an electrolytic cell containing AgNO_3 solution with inert electrodes. The weight of silver deposited was 1.50g . How long did the current flow ? (Molar mass of Ag=108 g " mol "^(-1), 1F=96500C " mol" ^(-1) ).

A current of 1.50 A was passed through an electrolytic cell containing AgNO_(3) solution with inert electrodes. The mass of the silver deposited at cathode was 1.50 g. How long did the current flow? (Atomic mass of Ag=108u, F=96500C).

Knowledge Check

  • If 965 coulombs of electricity is passed through a metal cup dipped in silver(l) salt solution, in order to plate it with silver. Then the amount of silver deposited on its surface is (Given : the molar mass of Ag = 108 g mol^(-1), 1F = 96500 coulombs)

    A
    `1.08 g`
    B
    `1.002 g`
    C
    `108 g`
    D
    `9.89 g`

  • A current of 2 ampere was passed through solutions of CuSO_4 and AgNO_3 in series. 0.635 g of copper was deposited. Then the weight of silver deposited will be-

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    0.59g
    B
    3.24g
    C
    1.08g
    D
    2.16g

  • A current of 2 ampere was passed through solutions of CuSO_(4) and AgNO_(3) in series . 0.635 g of copper was deposited . Then the weight of silver deposited will be

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    (a) A current of 1.50 amp was passed through an electrolytic cell containing AgNO_3 solution with inert electrodes. The weight of Ag deposited was 1.50 g. How long did the current flow ? (b) Write the reactions taking place at the anode and cathode in the above cell. (c) Give reactions taking place at the two electrodes if these are made up of Ag.

    (a) Current of 1.5 ampere was passed through an electrolyte containing AgNO_(3) solution with inert electrodes. The weight of silver deposited was 1.5 g. How long did the current flow ? (b) Write the reactions taking place at anode and at cathode in the above cell. (c ) Give the reactions taking place at the two electrodes if they are made up of silver.

    A constant current of 1.25 amperes is passed through an electrolytic cell containing a 0.05 M solution of CuSO_(4) and a copper anode and a platinum cathode until 1.58 g of copper is deposited . How long does the current flow to obtain 1.58 g of copper ?

    When a steady current of 2A was passed through two electrolytic cells A and B containing electrolytes ZnSO_4 and CuSO_4 connected in series, 2g of cu were deposited at the cathode of cell B. How long did the current flow? What mass of Zn was deposited at cathode of cell A?

    A steady current of 2 amperes was passed through two electrolytic cells X and Y connected in series containing electrolytes FeSO_(4) and ZnSO_(4) until 2.8 g of Fe deposited at the cathode of cell X. How long did the current flow? Calculate the mass of Zn deposited at the cathode of cell Y. (Molar mass : Fe=56 g"mol"^(-1)Zn=65.3"g mol"^(-1), F=96500"C mol"^(-1) )

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