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

Step-by-step solution

Given E^ _ Cd ²⁺| Cd = -0.403 V and E^ _ H ^+| H ₂ = 0.00 V . Since the standard reduction potential of cadmium is lower than that of hydrogen, cadmium has a higher tendency to get oxidized. Therefore, cadmium will act as the anode (oxidation) and the standard hydrogen electrode will act as the cathode (reduction). At anode: Cd _ (s) Cd ²⁺_ (aq) + 2 e ^- At cathode: 2 H ^+_ (aq) + 2 e ^- H _ 2(g) Adding the two half-cell reactions, the net cell reaction is: Cd _ (s) + 2 H ^+_ (aq) Cd ²⁺_ (aq) + H _ 2(g) Answer: Cd