1. What is Standard Cell Potential?

Definition: The standard cell potential is the potential difference between two half-cells under standard conditions (1M concentrations, 1 atm pressure, 25°C).

Purpose: It helps predict the direction of electron flow and the spontaneity of redox reactions in electrochemical cells.

2. How Does the Calculator Work?

The calculator uses the formula:

Where:

• \( E^\circ_{cell} \) — Standard cell potential (volts)
• \( \Delta G^\circ \) — Standard Gibbs free energy change (joules)
• \( n \) — Moles of electrons transferred in the redox reaction
• \( F \) — Faraday constant (96485.33212 C/mol)

Explanation: The negative of the Gibbs free energy change is divided by the product of moles of electrons and Faraday's constant.

3. Importance of Standard Cell Potential

Details: This calculation is fundamental in electrochemistry for determining cell voltages, predicting reaction spontaneity, and designing batteries.

4. Using the Calculator

Tips: Enter the standard Gibbs free energy change (ΔG°) in joules and moles of electrons transferred (n). The moles of electrons must be > 0.

5. Frequently Asked Questions (FAQ)

Q1: What does a positive E°_cell indicate?
A: A positive standard cell potential indicates a spontaneous reaction under standard conditions.

Q2: How do I find ΔG° for a reaction?
A: ΔG° can be calculated from standard formation energies or from the equation ΔG° = ΔH° - TΔS°.

Q3: What's the significance of the Faraday constant?
A: It represents the electric charge carried by one mole of electrons (approximately 96485 C/mol).

Q4: Can this calculator be used for non-standard conditions?
A: No, this calculates standard potential only. For non-standard conditions, use the Nernst equation.

Q5: What are typical values for standard cell potentials?
A: Most electrochemical cells have potentials between -3V and +3V, though some special cells may fall outside this range.