Standard Electrode Potential Formula
The standard electrode potential (E°) for a half-cell reaction can be calculated using the Nernst equation. The Nernst equation relates the standard electrode potential to the actual electrode potential under non-standard conditions. Hence, the formula for Standard Electrode Potential is given as:
E0 = E0cathode − E0anode
Where:
- E0cathode is the standard reduction potential of the cathode (reduction half-reaction).
- E0anode is the standard reduction potential of the anode (oxidation half-reaction).
Nernst Equation
Nernst equation is a fundamental equation in electrochemistry that relates the standard electrode potential of a cell to the actual cell potential under non-standard conditions. It is given as follows:
E = E∘– RT/nF ln Q
where:
- E is the cell potential under non-standard conditions.
- E is the standard cell potential
- R is the gas constant
- T is the temperature in Kelvin
- n is the number of moles of electrons transferred in the balanced redox reaction.
- F is the Faraday constant
- Q is the reaction quotient
Standard Electrode Potential
Standard electrode potential (E°) is a measure of the tendency of a half-reaction to occur as a reduction at a standard condition. In the context of standard electrode potential, “standard conditions” refer to a set of specific conditions under which the potential is measured. It includes standard concentration of all aqueous species to be 1 mol/L, pressure to be 1 atm and temperature to be 25℃ or 298K.
In this article, we will learn in detail about standard electrode potential, its formula, construction, factors affecting and applications.
Table of Content
- What is Standard Electrode Potential?
- Standard Electrode Potential Formula
- Construction of Standard Electrode Potential
- Difference Between Electrode Potential and Standard Electrode Potential
- Factors Affecting Electrode Potentials
- Standard Electrode Potential Example
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