If an electrochemical cell was made from Nickel and Iron, which metal would serve as the cathode and which as the anode?
Is the Fe dipping into a ferrous or a ferric solution? Let' say Fe^2+, Then
Fe(s) + Ni^2+(aq) ==> Fe^2+(aq) + Ni(s)
Oxidation occurs at the anode; reduction occurs at the cathode. So which is oxidized and which is reduced?
To determine which metal serves as the cathode and which as the anode in an electrochemical cell made from Nickel and Iron, you need to examine the reduction potentials of each metal. The metal with the higher reduction potential (more positive value) will act as the cathode, while the metal with the lower reduction potential (less positive value) will act as the anode.
Here's how you can find the reduction potentials:
1. Locate the reduction potentials for Nickel and Iron. You can refer to a table that provides standard reduction potentials.
2. Compare the reduction potentials of the two metals. The metal with the higher reduction potential will be the cathode, while the one with the lower reduction potential will be the anode.
For example, let's assume the reduction potentials for Nickel and Iron are:
- Nickel: -0.25 V
- Iron: -0.44 V
In this case, Nickel has the more positive reduction potential (-0.25 V), so it will serve as the cathode. Iron, with the less positive reduction potential (-0.44 V), will serve as the anode.
Remember, reduction potentials are used to determine the relative tendency of a metal to gain electrons (under standard conditions) and indicate its role as a cathode or anode in an electrochemical cell.