The following chemical reaction is occurring in an electrochemical cell,
`Mg(s) +2Ag^(+) (0.0001 M) to Mg^(2+) (0.10 M) +2Ag(s)`
`Mg^(2+) //Mg = -2.36V, Ag^(+)//Ag=0.81V`
For this cell calculate/write
(a) (i) `E^(Theta)` value for the electrode 2`Ag^(+)//2Ag`.
(ii) Standard cell potential `E_("cell")^(Theta)`
(b) Cell potential `(E )_("cell")`
(c ) (i) Symbolic representation of the above cell.
(ii) Will the above cell reaction be spontaneous ?

Explanation

To solve the given electrochemical cell problem step by step, we will follow the outlined parts of the question.

### Step-by-Step Solution

**(a) (i) Calculate E° for the electrode 2Ag⁺/2Ag:**

The standard reduction potential for the half-reaction \( \text{Ag}^+ + e^- \rightarrow \text{Ag} \) is given as \( E^\circ = 0.81 \, V \).

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