1. What is the Nernst Equation?

The Nernst equation calculates the reduction potential of an electrochemical cell or half-cell under non-standard conditions. It relates the measured potential to the standard potential and the activities (or concentrations) of the chemical species involved.

2. How Does the Calculator Work?

The calculator uses the Nernst equation:

Where:

• \( E \) — Reduction potential (V)
• \( E^0 \) — Standard reduction potential (V)
• \( R \) — Gas constant (8.314 J/mol·K)
• \( T \) — Temperature (K)
• \( n \) — Number of electrons transferred
• \( F \) — Faraday constant (96485.3329 C/mol)
• \( [ox] \) — Concentration of oxidized species (M)
• \( [red] \) — Concentration of reduced species (M)

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

3. Importance of Reduction Potential

Details: Reduction potential is crucial for understanding redox reactions, predicting reaction spontaneity, designing electrochemical cells, and studying biological electron transport chains.

4. Using the Calculator

Tips: Enter all required values with correct units. Concentrations must be positive, and temperature must be in Kelvin. Standard values are provided for R and F.

5. Frequently Asked Questions (FAQ)

Q1: What are standard conditions for E°?
A: Standard conditions are 298.15 K (25°C), 1 M concentration for solutions, and 1 atm pressure for gases.

Q2: How does temperature affect reduction potential?
A: Higher temperatures generally increase the effect of concentration changes on potential.

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

Q4: Can I use partial pressures for gases?
A: Yes, for gaseous species, you can substitute concentrations with partial pressures in atmospheres.

Q5: What is the significance of n in the equation?
A: n represents the number of electrons transferred in the redox half-reaction and significantly affects the potential.