1. What is the Nernst Equation?

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

2. How Does the Calculator Work?

The calculator uses the Nernst equation:

Where:

• \( E \) — Cell potential (V)
• \( E^0 \) — Standard cell potential (V)
• \( R \) — Gas constant (8.314 J/mol·K)
• \( T \) — Temperature (K)
• \( n \) — Number of electrons transferred
• \( F \) — Faraday's constant (96485 C/mol)
• \( [ox] \) — Concentration of oxidized species (M)
• \( [red] \) — Concentration of reduced species (M)

Explanation: The equation shows how cell potential changes with concentration and temperature.

3. Importance of Cell Potential Calculation

Details: Accurate cell potential calculation is crucial for predicting the feasibility of electrochemical reactions, designing batteries, and understanding corrosion processes.

4. Using the Calculator

Tips: Enter standard potential in volts, temperature in Kelvin, number of electrons transferred, and concentrations in molarity (M). All values must be positive.

5. Frequently Asked Questions (FAQ)

Q1: What is standard temperature for electrochemistry?
A: Most standard potentials are reported at 298K (25°C), but the calculator works for any temperature.

Q2: How does temperature affect cell potential?
A: Higher temperatures increase the effect of concentration differences on cell potential.

Q3: What if my concentrations are equal?
A: When [ox] = [red], the logarithm term becomes zero and E = E⁰.

Q4: Can I use this for non-standard conditions?
A: Yes, that's exactly what the Nernst equation is for - non-standard conditions.

Q5: What are typical values for standard potentials?
A: They range from about -3V to +3V depending on the half-reaction. Common values are tabulated in electrochemical series.