Cell Potential With Concentration Calculator

Nernst Equation:

\[ E = E^\circ - \frac{RT}{nF} \ln(Q) \]

Standard Potential E° (V):

Temperature T (K):

Moles n (mol):

mol

Faraday Constant F (C/mol):

C/mol

Reaction Quotient Q (dimensionless):

dimensionless

Cell Potential E (V):

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1. What is the Nernst Equation?

The Nernst equation calculates the cell potential of an electrochemical cell under non-standard conditions. It relates the measured cell potential to the standard cell potential and the reaction quotient, accounting for temperature and concentration effects.

2. How Does the Calculator Work?

The calculator uses the Nernst equation:

\[ E = E^\circ - \frac{RT}{nF} \ln(Q) \]

Where:

\( E \) — Cell potential (V)
\( E^\circ \) — Standard cell potential (V)
\( R \) — Universal gas constant (8.314 J/(mol·K))
\( T \) — Temperature (K)
\( n \) — Number of moles of electrons transferred (mol)
\( F \) — Faraday constant (96485 C/mol)
\( Q \) — Reaction quotient (dimensionless)

Explanation: The equation shows how the cell potential changes with concentration and temperature from the standard conditions.

3. Importance of Cell Potential Calculation

Details: Calculating cell potential is crucial for understanding electrochemical cells, battery performance, corrosion processes, and predicting the spontaneity of redox reactions under various conditions.

4. Using the Calculator

Tips: Enter standard potential in volts, temperature in Kelvin, moles of electrons transferred, Faraday constant, and reaction quotient. All values must be positive and valid.

5. Frequently Asked Questions (FAQ)

Q1: What is the significance of the reaction quotient Q?
A: The reaction quotient represents the ratio of product activities to reactant activities at any point in the reaction, indicating how far the reaction has progressed from equilibrium.

Q2: Why is temperature important in the Nernst equation?
A: Temperature affects the thermal energy available for electron transfer and influences the equilibrium constant, thus impacting the cell potential.

Q3: What are typical values for the Faraday constant?
A: The Faraday constant is approximately 96485 C/mol, representing the electric charge of one mole of electrons.

Q4: When does the Nernst equation predict zero cell potential?
A: When the reaction quotient Q equals the equilibrium constant K, the cell potential becomes zero, indicating the system is at equilibrium.

Q5: Can this calculator be used for concentration cells?
A: Yes, the Nernst equation applies to concentration cells where the standard potential is zero, and the cell potential depends solely on concentration differences.