Final answer:
To determine Faraday's constant, one must measure the electric charge in coulombs required to deposit or liberate one mole of substance during an electrochemical reaction, which involves measuring the current and time in an electrochemical cell and using Avogadro's number.
Step-by-step explanation:
To experimentally determine a value for Faraday's constant, one needs to know the amount of electric charge in coulombs required to deposit or liberate one mole of substance during an electrochemical reaction. During Faraday's experiments with electroplating, it was discovered that approximately 100,000 C per mole was needed to plate singly ionized ions. By dividing this charge by Avogadro's number, the charge per ion was approximated, and thus Faraday's constant was close to being calculated. In practice, to find Faraday's constant, one can measure the current (I) flowing through an electrochemical cell and the time (t) for which it flows. The total charge (Q) is the product of current and time, and when divided by the number of moles of electrons (n), gives Faraday’s constant (F).