Electrolysis Calculator
Calculate electroplating deposition mass, required current, or time using Faraday's Laws.
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Mastering Electrolysis with Faraday's Laws
Faraday's Laws of Electrolysis are the fundamental principles that govern how electrical energy converts chemical potential into mass. Discovered by Michael Faraday in 1834, these laws determine everything from the battery life of your smartphone to the chrome plating on your car.
Whether you are an industrial chemist calculating yield, a student solving stoichiometry problems, or a hobbyist electroplating jewelry, this calculator provides precise computations for Mass, Current, and Time.
Faraday's First Law
The First Law states that the chemical deposition due to the flow of current through an electrolyte is directly proportional to the quantity of electricity (Charge) passed through it.
Simply put: More Current + More Time = More Metal Plated.
Faraday's Second Law
The Second Law states that for the same quantity of electricity, the mass deposited is proportional to the Equivalent Weight of the substance.
Heavier atoms (high M) with low charge (low z) deposit the most mass per electron.
The Master Equation
Industrial Applications
Electroplating (Protective & Decorative)
The most common use. A thin layer of expensive or durable metal (like Gold, Silver, or Chromium) is deposited onto a cheaper base metal. This provides corrosion resistance (Chrome bumpers) or aesthetic appeal (Gold jewelry). Our tool helps jewelers calculate exactly how much gold is used, which is critical for costing.
Electrorefining (Purification)
Metals like Copper needs to be 99.99% pure for electrical wiring. Impure copper is used as the anode, and pure copper plate as the cathode. The impurities fall away as "anode mud", while pure copper atoms travel through the solution and deposit on the cathode.
Electrowinning (Mining)
Some highly reactive metals like Aluminum and Sodium cannot be extracted by standard heating with carbon. They must be "won" from their molten ores using electrolysis. This process consumes massive amounts of electricity, making calculation efficiency vital.
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Frequently Asked Questions
What is Faraday's Constant?
Faraday's Constant ($F \approx 96,485\ C/mol$) is a fundamental physical constant. It represents the total magnitude of electric charge carried by one mole of electrons. It connects determination of mass in chemistry to electrical measurements in physics.
What is Electrochemical Equivalent (Z)?
$Z$ is the mass of a substance deposited by 1 Coulomb of charge. It is equal to the Molar Mass divided by ($Valency \times Faraday's Constant$). Formula: $Z = M / (nF)$.
How does valency (z) affect deposition?
Valency is inversely proportional to mass. An ion with a charge of +2 (like Cu²⁺) requires twice as many electrons to neutralize than a +1 ion (like Ag⁺). Therefore, for the same current, you get half as many moles of Copper as Silver.
Why is my actual yield calculated vs real world different?
This is due to Current Efficiency. In reality, side reactions often occur (like the electrolysis of water generating Hydrogen gas). If efficiency is 90%, multiply your calculated mass by 0.90.
Does voltage affect the mass deposited?
Directly, no. Faraday's Law depends ONLY on Current (Amps) and Time. Voltage determines if the reaction can happen (must overcome the cell potential and overpotential), and it drives the current, but the math relies solely on charge ($Q = I \times t$).
Can I use this for gas production?
Yes! For example, estimating Hydrogen production. Remember that hydrogen gas is diatomic ($H_2$). So for $2H^+ + 2e^- \rightarrow H_2$, you need 2 moles of electrons to make 1 mole of gas.
What is the unit of 'Q'?
$Q$ is measured in Coulombs (C). One Coulomb is equal to one Ampere of current flowing for one Second ($1 C = 1 A \times 1 s$).
How do I calculate plating thickness?
First calculate the Mass ($m$). Then use the density formula: $Volume = Mass / Density$. Finally, $Thickness = Volume / Area$. You need to know the surface area of the object you are plating.
What is the difference between Electrolytic and Galvanic cells?
A Galvanic cell (battery) produces electricity from a spontaneous chemical reaction. An Electrolytic cell consumes electricity to force a non-spontaneous reaction (like plating) to occur. This calculator is for Electrolytic cells.
How do I convert Amp-Hours (Ah) to Coulombs?
1 Amp-Hour means 1 Amp flowing for 1 hour (3600 seconds). So, $1 Ah = 3600 Coulombs$.
Who was Michael Faraday?
Michael Faraday was a British scientist (1791–1867) who contributed significantly to the study of electromagnetism and electrochemistry. His main discoveries include electromagnetic induction, diamagnetism and electrolysis.
Does temperature affect the calculation?
Not directly in the formula. $F$, $M$, and $z$ are constants. However, temperature can affect the conductivity of the solution (resistance), which might change the Current ($I$) for a given Voltage, or improve Current Efficiency.