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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`

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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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