What are the half-reactions for a galvanic cell with aluminum and gold
electrodes?

The half-reactions for the galvanic cell with aluminum and gold electrodes is

Galvanic cells are electrochemical cells that generate electrical energy by the spontaneous activity in the oxidation-reduction (redox) reaction process.

The position of the metals if they are going to be at the cathode or at the anode relatively depends on the position with which they find themselves in the electrochemical series. The higher metal will be the anode and the lower metal in the electrochemical series will be the cathode.

Since aluminum is higher than gold on the electrochemical series, then:

Therefore, the half-reactions for the galvanic cell with aluminum and gold electrodes is

Learn more about Galvanic cells here:

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A

Explanation:

In a galvanic cell, energy is produced by spontaneous chemical processes.

The cathode and anode of this cell will depend on the relative position of the two metals in the electrochemical series.

Aluminium is higher in the electrochemical series so aluminium will be the anode. Silver is lower in the electrochemical series so silver will be the cathode.

Recall that oxidation (electron loss) occurs at the anode while reduction (electron gain) occurs at the cathode.

120,630,890

step-by-step explanation:

110+10=120,620+10=630,880+10=890