Which of the following net cell reactions occ | vedclass

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(B) $1$. The standard reduction potential of the standard hydrogen electrode $(SHE)$ is $E^0_{(H^+|H_2)} = 0.00 	ext{ V}$.$2$. The standard reduction

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$Cd(s) + 2H^+_{(aq)} \rightarrow Cd^{2+}_{(aq)} + H_2(g)$

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(B) $1$. The standard reduction potential of the standard hydrogen electrode $(SHE)$ is $E^0_{(H^+|H_2)} = 0.00 	ext{ V}$.$2$. The standard reduction potential of the cadmium electrode is $E^0_{(Cd^{2+}|Cd)} = -0.403 	ext{ V}$.$3$. Since $E^0_{(H^+|H_2)} > E^0_{(Cd^{2+}|Cd)}$, the hydrogen electrode acts as the cathode (reduction) and the cadmium electrode acts as the anode (oxidation).$4$. Anode reaction: $Cd(s) ightarrow Cd^{2+}_{(aq)} + 2e^-$.$5$. Cathode reaction: $2H^+_{(aq)} + 2e^- ightarrow H_2(g)$.$6$. Adding these two half-reactions gives the net cell reaction: $Cd(s) + 2H^+_{(aq)} ightarrow Cd^{2+}_{(aq)} + H_2(g)$.

Which of the following net cell reactions occurs in a galvanic cell containing a cadmium electrode and a standard hydrogen electrode? Given: $E^0_{(Cd^{2+}(aq)|Cd(s))} = -0.403 \text{ V}$.

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