Which of the following net cell reactions occ | vedclass

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(B) Step $1$: Identify the standard electrode potentials. For the standard hydrogen electrode $(SHE)$, $E^0(H^+|H_2) = 0.00 	ext{ V}$. For the cadmiu

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

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(B) Step $1$: Identify the standard electrode potentials. For the standard hydrogen electrode $(SHE)$, $E^0(H^+|H_2) = 0.00 	ext{ V}$. For the cadmium electrode, $E^0(Cd^{2+}|Cd) = -0.403 	ext{ V}$.Step $2$: Determine the anode and cathode. Since $E^0(Cd^{2+}|Cd) Step $3$: Write the half-reactions. Anode: $Cd(s) ightarrow Cd^{2+}(aq) + 2e^-$. Cathode: $2H^+(aq) + 2e^- ightarrow H_2(g)$.Step $4$: Combine the half-reactions to get 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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