Free Electrolysis Calculator

Electrolysis is an electrochemical process that forces a non‑spontaneous chemical reaction to occur by applying an electric current. The setup consists of two electrodes (anode and cathode), an electrolyte containing mobile ions, and an external power source. Electrons, each carrying a fundamental charge of approximately $1.602176634 \times 10^{-19}\ \text{C}$, flow from one electrode to the other, driving reduction at the cathode and oxidation at the anode.

Quantifying Mass Changes – Faraday’s First Law

The relationship between the amount of substance transformed at an electrode and the electric charge passed is described by Faraday’s first law of electrolysis. It states that the mass $m$ of a species deposited or dissolved is directly proportional to the total charge $Q$:

$$m = Z \cdot Q$$

Here $Z$ is the electrochemical constant (mass per unit charge), typically expressed in kg/C or g/C. Since charge can also be written as the product of current $I$ (amperes) and time $t$ (seconds), the equation becomes:

$$m = Z \cdot I \cdot t$$

What Is the Electrochemical Constant $Z$?

The constant $Z$ represents the mass of a substance that reacts when one coulomb of charge flows. It depends on the substance’s molar mass $M$, the number of electrons transferred per ion $n$, and Faraday’s constant $F \approx 96485\ \text{C/mol}$:

$$Z = \frac{M}{n \cdot F}$$

Tables of $Z$ values for common elements and compounds are available – this Electrochemistry Calculator includes a built‑in lookup so you don’t need to search manually.

Using the Faraday’s Law of Electrolysis Calculator

The tool is designed for convenience. Select the substance you are working with (e.g., copper, zinc, hydrogen, oxygen) or choose “Custom” to enter your own $Z$. Then input the electric charge – either directly in coulombs or as current and time with unit options (A, mA, h, min, etc.). The calculator instantly returns the expected mass change.

Example – Copper‑Zinc Cell

Consider a cell where a current of $0.1\ \text{A}$ flows for $60\ \text{s}$. The total charge is:

$$Q = 0.1\ \text{A} \times 60\ \text{s} = 6\ \text{C}$$

For copper, $Z_{\text{Cu}} \approx 3.294 \times 10^{-7}\ \text{kg/C}$; for zinc, $Z_{\text{Zn}} \approx 3.387 \times 10^{-7}\ \text{kg/C}$. The mass gained at the copper cathode (reduction) is:

$$m_{\text{Cu}} = Z_{\text{Cu}} \times 6\ \text{C} \approx 1.976 \times 10^{-6}\ \text{kg} = 1.976\ \text{mg}$$

The mass lost at the zinc anode (oxidation) is:

$$m_{\text{Zn}} = Z_{\text{Zn}} \times 6\ \text{C} \approx 2.032 \times 10^{-6}\ \text{kg} = 2.032\ \text{mg}$$

The calculator takes care of sign conventions based on the half‑reaction direction.

Example – Water Electrolysis

Water electrolysis splits $\text{H}_2\text{O}$ into hydrogen and oxygen gases. The Electrolysis Mass Calculator provides the constants for $\text{H}_2$ and $\text{O}_2$. If you use a phone battery with a capacity of $4000\ \text{mAh}$ as the power source, the charge is:

$$Q = 4000\ \text{mAh} \times 3.6 = 14400\ \text{C}$$

Using $Z_{\text{H}_2} \approx 1.045 \times 10^{-8}\ \text{kg/C}$, the mass of hydrogen produced is:

$$m_{\text{H}_2} \approx 1.045 \times 10^{-8} \times 14400 \approx 1.505 \times 10^{-4}\ \text{kg} = 150.5\ \text{mg}$$

For oxygen, $Z_{\text{O}_2} \approx 8.291 \times 10^{-8}\ \text{kg/C}$:

$$m_{\text{O}_2} \approx 8.291 \times 10^{-8} \times 14400 \approx 1.194 \times 10^{-3}\ \text{kg} = 1.194\ \text{g}$$

These figures show that even a modest portable battery can generate measurable amounts of gas, highlighting the relevance of electrolysis in clean energy research.

Why This Tool Is Useful

Whether you are a student studying Faraday’s First Law, a hobbyist experimenting with electroplating, or a researcher designing an electrolytic cell, this Mass of Substance Produced Calculator eliminates manual errors and speeds up your work. It serves as both a dedicated Faraday’s Law of Electrolysis Calculator and a handy Electrochemical Constant Calculator. By focusing on the science rather than the arithmetic, you can quickly explore “what‑if” scenarios and confirm experimental expectations.

In summary, electrolysis bridges chemistry and electricity through the simple but powerful relation $m = Z Q$. With this tool, you can apply that relation to any common electrode material or even define your own constant, making it an indispensable companion for electrochemistry calculations.