Consider the reaction `2Ag^(+) + Cd to 2Ag + Cd^(2+)`. The standard reduction potentials of `Ag^(+)//Ag and Cd^(2+)//Cd are + 0*80 " volt and " 0*40` volt, respectively.
Will the cell work spontaneously for the condition given in (iii) above?

Explanation

To determine if the cell will work spontaneously for the given reaction \(2Ag^+ + Cd \rightarrow 2Ag + Cd^{2+}\), we need to analyze the standard reduction potentials of the half-reactions involved.

### Step 1: Identify the half-reactions
The half-reactions for the given reaction are:
1. Reduction half-reaction: \(Ag^+ + e^- \rightarrow Ag\)
2. Oxidation half-reaction: \(Cd \rightarrow Cd^{2+} + 2e^-\)

### Step 2: Write the standard reduction potentials
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