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How much time approximately would it tak...

How much time approximately would it take in minutes to deposit 1.18 g of metallic copper on a metal object when a current of 2.0 A is passed through the electrolytic cell containing `Cu^(2+)` ions?

A

10 min

B

20 min

C

30 min

D

40 min

Text Solution

Verified by Experts

The correct Answer is:
C
According to Faraday.s first law:
w=Zit
w=1.18 g. z= `63.5/(2xx96500) ` , I=2 A
t= `w/(ZI)=1.18/(63.5xx2)xx2xx96500=1793` s or `1793/60~~30 m`
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Knowledge Check

  • Time required to deposit one millimole of aluminium metal by the passage of 9.65 amperes through molten electrolyte containing aluminium ion is

    A
    30 s
    B
    10 s
    C
    30,000 s
    D
    10,000 s

  • The number of moles of electrons passed when current of 2 A is passed through an solution of electrolyte for 20 minutes is ___________.

    A
    `4.1 xx 10^(-4) " mol " e^(-)`
    B
    `1.24 xx 10^(-2)" mol "e^(-)`
    C
    `2.487 xx 10^(-2)" mol "e^(-)`
    D
    `2.487 xx 10^(-1)" mol "e^(-)`

  • Calculate the weight of metal deposited when a current of 15 ampere with 75% current efficiency is passed through the cell for 2 hours. (Electrochemical equivalent of metal = 4xx10^(-4) )

    A
    32.4 g
    B
    43.2 g
    C
    57.6 g
    D
    16.2 g

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