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Represent the cell in which the followin...

Represent the cell in which the following reaction takes place
`Mg(s)+2Ag^(+)(0.0001M) to Mg^(2+) (0.130M)+2Ag(s)`
Calculates its `E_(cell)` if `E_("cell")^(Θ)=3.17V`

Text Solution

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The correct Answer is:
2.96 v
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Mg(s) + 2Ag^(+)(0.0001M) to 2Ag(s) + Mg^(2+) (0.13 M) . Calculate the E_("cell") is given as 3.17 V.

Calculate the emf of the cell with the cell reaction Ni _((s))+2Ag ^(+)(0.002M)to Ni^(2+)(0.160M) +2 Ag_((s)) E_(cell)^(0)=1.05V.

Knowledge Check

  • If E_(cell)^(@) is 1.05 V, the emf of the cell for the following cell reaction Ni(s)+2Ag^(+)(0.004 M) rarr Ni^(2+)(0.16M)+2Ag(s) at 298 K in V is

    A
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    B
    1.227
    C
    0.732
    D
    1.397

  • The emf of the cell in which of the following reaction , Zn_((s)) +Ni^(2+) (0.1 M) to Zn^(2+) (1.0M) + Ni_((s)) occurs is found to 0.5105 V at 298 K . The standard emf of the cell is

    A
    `0.4810 V `
    B
    `0.5696 V `
    C
    `-0.5105 V `
    D
    `0.5400 V `

  • For the redox reaction : Zn(s) + Cu^(2+) (0.1M) to Zn^(2+) (1M) + Cu(s) taking place in a cell, E_("cell")^@ is 1.10 volt. E_("cell") for the cell will be

    A
    2.14 volt
    B
    1.07 volt
    C
    1.80 volt
    D
    0.82 volt

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