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Calculate the e.m.f of the cell Mg(s)/...

Calculate the e.m.f of the cell
`Mg(s)//Mg^(2+)(0.1 M)||Cu^(2+)(1.0xx10^(-3) M)//Cu(s)`
Given `E_(Cu^(2+)//Cu)^(@)=+0.34 V` and `E_(Mg^(2+)//Mg)^(@)=-2.37 V`

Text Solution

AI Generated Solution

To calculate the e.m.f of the cell `Mg(s)//Mg^(2+)(0.1 M)||Cu^(2+)(1.0xx10^(-3) M)//Cu(s)`, we will follow these steps: 1. **Identify the half-reactions at the anode and cathode**: - Anode (oxidation): `Mg(s) -> Mg^(2+)(aq) + 2e^-` - Cathode (reduction): `Cu^(2+)(aq) + 2e^- -> Cu(s)` 2. **Determine the standard electrode potentials**: - Given: `E_(Cu^(2+)//Cu)^(@) = +0.34 V` ...
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Knowledge Check

  • Calculate the emf of the following cell at 298K: Mg(s)|Mg^(2+)(0.1M)||Cu^(2+)(1.0xx10^(-3)M)|Cu(s) [Given= E_(Cell)^(@)=2.71V ]

    A
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    B
    2.503V
    C
    2.651 V
    D
    1.8V

  • The standard cell potential for the cell Zn|Zn^(2+) (1 M)|| Cu^(2+) (1 M)| Cu Given E_(Cu^(2+)//Cu)^(@) = 0.34 V and E_(Zn^(2+)//Zn)^(@) = - 0.76 V is

    A
    1.10 V
    B
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    C
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    D
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