Determine whether `O_(2)(g)` can oxidize sulphate `(SO_(4)^(2-))` ion to peroxodisulphate `(S_(2)O_(8)^(2-))` ion in an acidic solution with `O_(2)(g)` being reduced to water.
Given `: E^(c-)._(O_(2)|H_(2)O)=1.20V` and `E^(C-)._(S_(2)O_(8)^(2-)|2SO_(4)^(2-))=2.0V`

Explanation

To determine whether \( O_2(g) \) can oxidize sulfate \( (SO_4^{2-}) \) ion to peroxodisulfate \( (S_2O_8^{2-}) \) ion in an acidic solution, we need to analyze the standard reduction potentials provided and apply the concept of cell potential.

### Step 1: Write the half-reactions
1. The reduction half-reaction for oxygen:
\[ O_2(g) + 4H^+ + 4e^- \rightarrow 2H_2O \quad (E^\circ = 1.20 \, V) \]

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