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How would you determine the standard ele...

How would you determine the standard electrode potential of the system `Mg^(2+)//Mg?`

Text Solution

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`E^(0)` vlaue of `Mg^(2+)//Mg` electrode is determined by setting up an electrochemical cell. For this purpose, a Mg electrode is dipped in `1 M Mg SO_(4)` solution, which acts as one half cell i.e., oxidation half-cell.
In the same way, the standard hydrogen electrode acts as the other half-cell i.e., reduction half cell. The deflection of voltmeter placed in the cell circuit is towards the Mg electrode which indicates the direction of flow of current.
The cell may be represented as : `Mg|Mg^(2+)(1M)||H^(+)(M)|H_(2) (1 atm).` Pt The reading as given by boltmeter gives `E_(cell)^(0)`
`E_(cell)^(0) =E_((H^(+)//1//2H_(2)))^(0) -E_((Mg^(2+)//Mg))^(0) =0-E_((Mg^(2+)//Mg))^(0)`
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Knowledge Check

  • Which defines the standard reduction electrode potential of Zn^(2+) ions?

    A
    `Zn_((aq))^(2+) + 2e to Zn_((s)) , [Zn^(2+)] = 1 M`
    B
    `Zn_((g)) to Zn^(2+) + 2e , [Zn^(2+)] = 1M `
    C
    `Zn_((aq))^(2+) to Zn_((s)) + 2e , [Zn^(2+) ] = 1M `
    D
    `Zn_((g))^(2+) to Zn_((s)) - 2e , [Zn^(2+)] = 1M`

  • The standard reduction potential of Cu^(2+) // Cu and Cu^(+) // Cu are 0.337 and 0.153 V respectively . The standard electrode poetential of Cu^(2+) // Cu^(+) half cell will be

    A
    `0.184 V `
    B
    `0.827V `
    C
    `0.521 V `
    D
    `0.490V `

  • A standard hydrogen electrode has zero electrode potential because

    A
    Hydrogen is easiest to oxidise
    B
    This electrode potential is assumed to be zero
    C
    Hydrogen atom has only one electron
    D
    Hydrogen is the lightest element

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