For a Galvanic cell consisting of a zinc electrode and a standard hydrogen electrode,$E^{\circ}(Zn^{+2}_{(aq)} \mid Zn_{(s)}) = -0.76 \ V$. Identify the reaction that takes place at the positive electrode during the working of the cell.
- A$Zn_{(s)} \longrightarrow Zn^{+2}_{(aq)} + 2e^{-}$
- B$Zn^{+2}_{(aq)} + 2e^{-} \longrightarrow Zn_{(s)}$
- C$H_{2(g)} \longrightarrow 2H^{+}_{(aq)} + 2e^{-}$
- D$2H^{+}_{(aq)} + 2e^{-} \longrightarrow H_{2(g)}$
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