In electrochemistry, the **Nernst equation** is an equation that can be used (in conjunction with other information) to determine the equilibrium reduction potential of a half-cell in an electrochemical cell. It can also be used to determine the total voltage (electromotive force) for a full electrochemical cell. It is named after the German physical chemist who first formulated it, Walther Nernst.

The Nernst equation gives a formula that relates the numerical values of the concentration gradient to the electric gradient that balances it. For example, if a concentration gradient was established by dissolving KCl in half of a divided vessel that was originally full of H_{2}O, and then a membrane permeable to K+ ions was introduced between the two halves—empirically, an equilibrium situation would arise where the chemical concentration gradient (that would normally cause ions to move from the region of high concentration to the region of low concentration) could be balanced by an electrical gradient that opposes the movement of charge.

Read more about Nernst Equation: Expression, Nernst Potential, Relation To Equilibrium, Limitations

### Other articles related to "nernst equation, equation":

**Nernst Equation**

... For a half cell

**equation**, conventionally written as reduction (electrons on the left side) where is the standard Gibbs free energy change, is the number of electrons involved, and is Faraday's constant ... The

**Nernst equation**relates pH and where curly brackets indicate activities and exponents are shown in the conventional manner ... This

**equation**is the

**equation**of a straight line for as a function of pH with a slope of volt (pH has no units.) This

**equation**predicts lower at higher pH values ...

**Nernst Equation**

... In electrochemistry, the

**Nernst equation**is an

**equation**which can be used (in conjunction with other information) to determine the equilibrium reduction potential of a ...

... the cell was reduced as predicted using the

**Nernst equation**for the model ... The Nerst

**equation**essentially says how much the voltage drops as more zinc sulfate is added ... This effect is also predicted by the

**Nernst equation**the particular acid that was used (citric, hydrochloric, sulfuric, etc.) doesn't affect the voltage except through the pH value ...

**Nernst Equation**- Limitations

... In dilute solutions, the

**Nernst equation**can be expressed directly in terms of concentrations (since activity coefficients are close to unity) ... This complicates the use of the

**Nernst equation**, since estimation of non-ideal activities of ions generally requires experimental measurements ... The

**Nernst equation**also only applies when there is no net current flow through the electrode ...

... It can be calculated using the

**Nernst equation**where Eeq,K+ is the equilibrium potential for potassium, measured in volts R is the universal gas constant, equal to 8.314 joules·K−1·mol−1 T is the absolute ... Applying the

**Nernst Equation**above, one may account for these differences by changes in relative K+ concentration or differences in temperature ... For common usage the

**Nernst equation**is often given in a simplified form by assuming typical human body temperature (37 C), reducing the constants and switching to Log base 10 ...

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