1. What is EMF of Concentration Cell without Transference?

Definition: The electromotive force (EMF) of a concentration cell is the potential difference developed between two half-cells with different concentrations of the same electrolyte.

Purpose: This calculator helps determine the EMF for dilute solutions where ion transference between half-cells is negligible.

2. How Does the Calculator Work?

The calculator uses the Nernst equation for concentration cells:

Where:

• \( EMF \) — Electromotive force (volts)
• \( [R] \) — Universal gas constant (8.314 J/mol·K)
• \( T \) — Temperature (Kelvin)
• \( [Faraday] \) — Faraday constant (96485 C/mol)
• \( c2 \) — Cathodic concentration (mol/m³)
• \( c1 \) — Anodic concentration (mol/m³)

Explanation: The formula calculates the potential difference created by the concentration gradient of ions in the cell.

3. Importance of EMF Calculation

Details: Accurate EMF calculation is crucial for understanding electrochemical cell behavior, designing batteries, and corrosion studies.

4. Using the Calculator

Tips: Enter the temperature in Kelvin and both concentrations in mol/m³. All values must be positive numbers.

5. Frequently Asked Questions (FAQ)

Q1: What is a concentration cell?
A: An electrochemical cell that generates voltage from a concentration difference of the same electrolyte solution.

Q2: Why multiply by 2 in the formula?
A: The factor of 2 accounts for the two electrons transferred in the redox reaction of a typical concentration cell.

Q3: What temperature range is valid?
A: The formula works for any temperature above absolute zero, but standard calculations typically use 298K (25°C).

Q4: What if concentrations are equal?
A: The EMF will be zero since ln(1) = 0, indicating no concentration gradient to drive the cell.

Q5: How does temperature affect EMF?
A: Higher temperatures generally increase EMF for a given concentration ratio, as seen in the direct proportionality to T.