1. What is Standard Reduction Potential?

Standard reduction potential (E°) measures the tendency of a chemical species to be reduced. The standard cell potential (E°_cell) is the difference between the reduction potentials of the cathode and anode.

2. How Does the Calculator Work?

The calculator uses the standard cell potential equation:

Where:

• \( E_{cell} \) — Standard cell potential (volts, V)
• \( E_{cathode} \) — Reduction potential of cathode (V)
• \( E_{anode} \) — Reduction potential of anode (V)

Explanation: The equation shows that cell potential depends on the difference between the reduction potentials of the two half-cells.

3. Importance of Standard Cell Potential

Details: The standard cell potential predicts whether a redox reaction will occur spontaneously (positive E°_cell) and determines the maximum potential difference of an electrochemical cell.

4. Using the Calculator

Tips: Enter standard reduction potentials for both half-reactions in volts (V). The cathode is the reduction half-reaction, and the anode is the oxidation half-reaction (use the reduction potential value).

5. Frequently Asked Questions (FAQ)

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

Q2: How do I know which is cathode and anode?
A: The cathode is where reduction occurs (higher reduction potential), and the anode is where oxidation occurs (lower reduction potential).

Q3: What are standard conditions?
A: 25°C (298K), 1 atm pressure, and 1M concentration for all solutions.

Q4: Can I use this for non-standard conditions?
A: No, this calculates standard potential only. Use the Nernst equation for non-standard conditions.

Q5: Where can I find standard reduction potentials?
A: Standard reduction potential tables are available in chemistry references and textbooks.