$A$ galvanic cell consists of a copper electrode and a standard hydrogen electrode. If $E^\circ (Cu^{2+}_{(aq)} | Cu_{(s)}) = +0.34 \text{ V}$, identify the reaction taking place at the positive electrode during the working of the cell.
- A$Cu_{(s)} \longrightarrow Cu^{2+}_{(aq)} + 2e^-$
- B$Cu^{2+}_{(aq)} + 2e^- \longrightarrow Cu_{(s)}$
- C$H_2(g) \longrightarrow 2H^+_{(aq)} + 2e^-$
- D$H^+_{(aq)} + 2e^- \longrightarrow H_2(g)$
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$Sn^{4+} + 2e^- \to Sn^{2+}; E^o = 0.1 \ V$
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