It seems to be working again. My question is why they subtract the iron cell potential. The reduction potential is negative, so to change it to oxidation potential would it not become positive, and then you add it to the cathodes cell potential?mjc123 said:
A galvanic cell is an electrochemical cell that uses spontaneous redox reactions to generate electrical energy. It consists of two half-cells, each containing an electrode and an electrolyte solution, connected by a salt bridge.
In a galvanic cell, iron oxidation occurs at the anode, where the iron electrode is oxidized and releases electrons into the external circuit. These electrons flow through the circuit to the cathode, where reduction of a different species (such as oxygen) occurs.
The rate of iron oxidation in a galvanic cell can be affected by several factors, including the concentration of the electrolyte solution, the surface area of the iron electrode, and the temperature of the cell. Higher concentrations and surface areas, as well as higher temperatures, generally result in faster rates of iron oxidation.
Iron oxidation is important in a galvanic cell because it is the source of the electrical energy produced by the cell. The flow of electrons from the anode to the cathode creates a current that can be harnessed for practical uses.
To solve a galvanic cell problem involving iron oxidation, you will need to use the principles of electrochemistry to balance the redox reactions occurring at the anode and cathode. This involves using the Nernst equation to calculate the cell potential and the standard reduction potentials of the species involved. Practice and familiarity with these concepts will help you successfully solve galvanic cell problems involving iron oxidation.