The Faraday Constant Calculator is a simple yet powerful tool designed to compute the total electric charge carried by one mole of electrons. It helps users convert fundamental constants into a usable value for applications in chemistry, electrochemistry, and physics. The result gives the Faraday constant, which is a vital link between the amount of substance and the electric charge involved in redox reactions and electrolysis processes.
This calculator is part of the Physics and Chemistry Constants Calculators category. It supports researchers, students, and professionals by providing an accurate way to derive the Faraday constant using known values of Avogadro’s number and the elementary charge.
formula of Faraday Constant Calculator
Faraday Constant (F) = N_A × e
Where:
F = Faraday Constant (in coulombs per mole, C/mol)
N_A = Avogadro’s number = 6.02214076 × 10²³ mol⁻¹
e = Elementary charge = 1.602176634 × 10⁻¹⁹ C
So, using the formula:
F = (6.02214076 × 10²³ mol⁻¹) × (1.602176634 × 10⁻¹⁹ C)
F ≈ 96485.332123 C/mol
This means one mole of elementary charges carries approximately 96485 coulombs of charge.
Reference Table for Common Values
Constant Name | Symbol | Value | Unit |
---|---|---|---|
Avogadro’s Number | N_A | 6.02214076 × 10²³ | mol⁻¹ |
Elementary Charge | e | 1.602176634 × 10⁻¹⁹ | C |
Faraday Constant | F | 96485.332123 | C/mol |
One mole of electrons | - | Carries 96485.33 | Coulombs |
This table is useful for quick referencing in scientific reports, academic study, or laboratory use.
Example of Faraday Constant Calculator
Let’s say you want to verify the Faraday constant using known values.
Step 1: Write down the known values
N_A = 6.02214076 × 10²³ mol⁻¹
e = 1.602176634 × 10⁻¹⁹ C
Step 2: Plug into the formula
F = N_A × e
F = (6.02214076 × 10²³) × (1.602176634 × 10⁻¹⁹)
Step 3: Calculate
F ≈ 96485.332123 C/mol
So, the Faraday constant is about 96485.33 coulombs per mole.
Most Common FAQs
It is use to relate the electric charge to the amount of substance (in moles) in electrochemical reactions. It’s essential in calculating how much substance is oxidize or reduced in a reaction involving electricity.
Because it helps determine how much charge is need to deposit or dissolve a certain mass of material at an electrode, making it vital for battery design and chemical manufacturing.
The value of the Faraday constant stays consistent but is typically expressed in C/mol. Its components (N_A and e) are both SI units, so the result is also in SI terms unless unit conversions are applied.