User:OITowl3/sandbox

Original text

Each half-reaction has a standard electrode potential (E⁰_cell), which is the voltage generated from the reaction at equilibrium under standard conditions of an electrochemical cell.

The electrode potential of each half-reaction is also known as its reduction potential E⁰_red, or potential when the half-reaction takes place at a cathode. The reduction potential is a measure of the tendency of the oxidizing agent to be reduced. H⁺ has a reduction potential of zero, the values of oxidizing agents that are stronger than H⁺ are positive and the values of oxidizing agents that are weaker than H⁺ are negative.

For a redox reaction which takes place in a cell, the potential difference E⁰_cell = E⁰_cathode – E⁰_anode

Revised text

Each half-reaction has a standard electrode potential (E⁰_cell), which is the voltage generated from the reaction at equilibrium under standard conditions of an electrochemical cell.

The electrode potential of each half-reaction is also known as its reduction potential E⁰_red, or potential when the half-reaction takes place at a cathode. The reduction potential is a measure of the tendency of the oxidizing agent to be reduced. H⁺ has a reduction potential of zero, the values of oxidizing agents that are stronger than H⁺ are positive and the values of oxidizing agents that are weaker than H⁺ are negative.

For a redox reaction which takes place in a cell, the potential difference E⁰_cell = E⁰_cathode – E⁰_anode

Comments

I liked that the first paragraph was shortened, it's original version had too much unneeded information. I also think an example of how to find the electric potential would be useful, otherood than that it's good. Tree19 (talk) 22:26, 2 June 2013 (UTC)