Solve Galvanic Cell Problem: Iron Oxidation

In summary, the conversation discusses a misunderstanding about the process of subtracting and adding cell potentials in an oxidation reaction. The question is about whether or not the iron cell potential should be flipped and added to the cathode's potential. The response clarifies that the iron potential should be subtracted from the higher potential or the half-equation should be flipped and the numbers added. The final equation given in the textbook is incorrect.
  • #1
Chemistry314
2
0
DXrMA02.jpg

http://imgur.com/a/wGTEQ

The example is straight from my textbook. Since the iron is being oxidized, and it has a negative cell potential to begin with, wouldn't you flip the equation to make it the anode and in the end add it to the other cell potential?
 
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  • #2
No image. Write out your question.
 
  • #3
mjc123 said:
No image. Write out your question.
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?
 
  • #4
Yes. The textbook is not very clear here, and the final equation is actually wrong. You should either
Subtract the lower reduction potential from the higher (this is the easiest way), or
Flip round the half-equation with the lower reduction potential, reverse the sign (to make it an oxidation potential) and add the two numbers.
Either way you get Eocell = 1.51 - (-0.44) = 1.95V
 

FAQ: Solve Galvanic Cell Problem: Iron Oxidation

What is a galvanic cell?

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.

How does iron oxidation occur in a galvanic cell?

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.

What factors affect the rate of iron oxidation in a galvanic cell?

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.

What is the significance of iron oxidation in a galvanic cell?

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.

How can I solve a galvanic cell problem involving iron oxidation?

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.

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