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

Explanation

In order to determine `E^(@)` value of `Mg^(2+)//Mg` electrode, an electrochemical cell is set up in which a Mg electrode dipped in 1 M `MgSO_(4)` solution acts as one half cell (oxidation half cell) while the standard hydrogen electrode acts as the other half cell (reduction half cell). The deflection of voltmeter placed in the cell circuit is towards the Mg-electrode indicating the flow of current. The cell may be represented as :
`Mg//Mg^(2+)(1 M)|| H^(+)(1 M)//H_(2)(1 atm)`,
The reading as given by voltmeter gives `E_(cell)^(@)`
`E_(cell)^(@)=E_(H^(+)//1//2H_(2))^(@)-E_(Mg^(2+)//Mg)^(@)=0-E_(Mg^(2+)//Mg)^(@)`
The expected value of standard electrode potential (`E^(@)`)=-2.36 V`.