Electrolysis & Electroplating Solver

Electrolysis & Faraday's Laws

**Electrolysis** is a process that uses direct electric current (DC) to drive an otherwise non-spontaneous chemical reaction. This is commercially important in the separation of elements from naturally occurring sources.

Faraday's 1st Law: $W = Z \cdot I \cdot t$
Mass Liberated: $W = \frac{E \cdot I \cdot t}{96500}$

Calculate Mass Liberated ($W$)

Equivalent Weight ($E$) [At. Mass / Valency] Current ($I$) in Amperes Time ($t$) in Seconds

Calculate Time Required ($t$)

Mass to be deposited ($W$) in grams Equivalent Weight ($E$) Current ($I$) in Amperes

Calculate Current Intensity ($I$)

Mass Deposited ($W$) in grams Equivalent Weight ($E$) Time ($t$) in Seconds

Charge & Faraday Count

Current ($I$) in Amperes Time ($t$) in Seconds

Electroplating Thickness

Mass Deposited ($W$) in grams Surface Area ($A$) in $cm^2$ Density of Metal ($\rho$) in $g/cm^3$

Thickness ($d$) = $\frac{W}{A \cdot \rho}$

Guide: Entering Values

Our calculators use a smartParser to handle scientific notation.

Exponent: 10^5 means 10⁵

Multiply: 10*1 means 10 multiplied by 1.

Scientific: 1.8e-5 means 1.8 × 10^-5

Practical Examples:

Positive: Enter 10^2 for 100.
Negative: Enter -5 for acidic values.
Complex: Enter 10^-7 for neutral pH.

What is Electrolysis?

Electrolysis is the decomposition of an electrolyte by the passage of an electric current. It occurs in an **Electrolytic Cell**, where electrical energy is converted into chemical energy.

How it Works

When the DC power supply is turned on:

Cations (+): Migrate toward the negative electrode (**Cathode**) and gain electrons (Reduction).
Anions (-): Migrate toward the positive electrode (**Anode**) and lose electrons (Oxidation).

The total amount of chemical change is directly proportional to the quantity of electricity passed.

Applications

Electroplating: Coating a cheap metal with a layer of a precious metal (Gold, Silver, Chromium).
Extraction of Metals: Producing Reactive metals like Aluminum (Hall-Héroult process) and Sodium.
Refining: Purifying metals like Copper to 99.99% purity.

Solved Examples

Example 1: A current of 0.5A is passed through $CuSO_4$ for 30 mins. Find the mass of Cu deposited. ($E=31.75$)
$W = (31.75 \times 0.5 \times 1800) / 96500 = 0.296$ g.

Example 2: How many Coulombs are required to deposit 1 mole of $Al$ from $Al^{3+}$?
Since $n=3$, Charge = $3 \times 96500 = 289,500$ C.

Scientific Research & Green Energy

Electrolysis is at the heart of the "Hydrogen Economy." Researchers are focusing on:

Water Electrolysis: Splitting water into Hydrogen and Oxygen using renewable energy (Solar/Wind).
Carbon Capture: Using electrolytic cells to convert atmospheric $CO_2$ into useful fuels.
Nanotechnology: Electro-deposition of nanowires for next-gen semiconductors.

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