The standard cell notation for an electrolytic cell with aluminum and gold electrodes is (c) (aq) | Au(s) || Al(s) | (aq). The half-cell reactions occurring in this electrolytic cell are: Anode: Al(s) -> (aq) + 3e- and Cathode: (aq) + 3e- -> Au(s). The correct answer is option C.
The standard cell notation (c) (aq) | Au(s) || Al(s) | (aq) represents an electrolytic cell where aluminum (Al) and gold (Au) electrodes are involved. In this notation, the left side of the double vertical line (||) signifies the anode, and the right side represents the cathode.
At the anode (Al(s)), aluminum undergoes oxidation, losing electrons to form aluminum ions (Al3+): Al(s) → (aq) + 3e-. This reaction occurs at the anode, and electrons flow from the anode to the cathode.
At the cathode ((aq)), gold ions gain electrons and are reduced to form solid gold (Au(s)): (aq) + 3e- → Au(s). This reduction reaction takes place at the cathode, where electrons received from the anode contribute to the reduction of gold ions.
The notation follows the standard convention where the species in the same phase are grouped together and the anode is written before the cathode. This cell notation provides a concise representation of the redox reactions occurring in the electrolytic cell involving aluminum and gold electrodes.
Oxidation takes place at the anode. Reduction takes place at the cathode. Oxidation takes place on the left and recution takes place on the right.
The standard cell notation for an electrolytic cell with alumium and gold electrodes:
To determine which metal undergoes oxidation and which undergoes reduction we use the standard cell potentetial of the metals. Au is the stronger oxidising agent of the two and so it is likely to undergo reduction and so the Al will undergo oxidation.
Answer: A
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