Calculate the mass of substance produced or consumed during electrolysis by entering current, time, and electrode material. Based on Faraday's Law of Electrolysis for accurate electrochemical calculations.
Molar mass: 63.55 g/mol,Valency: 2,Used in electrical wiring and plating
Results update automatically as you change values
Calculate precise electrolysis mass deposition with our free online calculator using Faraday's Law. Perfect for electroplating, metal refining, and electrochemistry applications.
Electrolysis is a fundamental electrochemical process that uses electrical current to drive non-spontaneous chemical reactions. This Electrolysis Calculator applies Faraday's Law to accurately determine the mass of substance produced or consumed at an electrode during electrolysis. Whether you're a student learning electrochemistry, a researcher conducting experiments, or an industrial engineer optimizing electroplating processes, this calculator provides a straightforward way to predict the amount of material deposited or dissolved during electrolysis.
Faraday's Law of Electrolysis establishes the quantitative relationship between the amount of electrical charge passed through an electrolyte and the amount of substance transformed at an electrode. This principle forms the backbone of numerous industrial applications, including electroplating, electrorefining, electrowinning, and the production of high-purity chemicals.
Our calculator allows you to input the current (in amperes), time duration (in seconds), and select from common electrode materials to instantly calculate the mass of substance produced or consumed during the electrolysis process. The intuitive interface makes complex electrochemical calculations accessible to users at all levels of expertise.
Faraday's Law of Electrolysis states that the mass of a substance produced at an electrode during electrolysis is directly proportional to the quantity of electricity transferred at that electrode. The mathematical formula is:
Where:
Since electric charge can be calculated as current multiplied by time (), the formula can be rewritten as:
Where:
Current (I): The flow of electric charge, measured in amperes (A). In electrolysis, current represents the rate at which electrons flow through the circuit.
Time (t): The duration of the electrolysis process, typically measured in seconds. For industrial applications, this might be hours or days, but the calculation converts to seconds.
Molar Mass (M): The mass of one mole of a substance, measured in grams per mole (g/mol). Each element has a specific molar mass based on its atomic weight.
Valency Number (z): The number of electrons transferred per ion during the electrolysis reaction. This depends on the specific electrochemical reaction occurring at the electrode.
Faraday Constant (F): Named after Michael Faraday, this constant represents the electric charge carried by one mole of electrons. Its value is approximately 96,485 coulombs per mole (C/mol).
Let's calculate the mass of copper deposited when a current of 2 amperes flows for 1 hour through a copper sulfate solution:
Therefore, approximately 2.37 grams of copper will be deposited at the cathode during this electrolysis process.
Our Electrolysis Calculator is designed to be intuitive and user-friendly. Follow these steps to calculate the mass of substance produced or consumed during electrolysis:
Electrolysis calculations have numerous practical applications across various fields:
Electroplating involves depositing a thin layer of metal onto another material using electrolysis. Precise calculations are essential for:
Example: A jewelry manufacturer needs to deposit a 10-micron layer of gold on silver rings. Using the electrolysis calculator, they can determine the exact current and time required to achieve this thickness, optimizing their production process and reducing gold wastage.
Electrolysis is crucial in extracting and purifying metals:
Example: A copper refinery uses electrolysis to purify copper from 98% to 99.99% purity. By calculating the precise current needed per ton of copper, they can optimize energy consumption and maximize production efficiency.
Electrolysis calculations are fundamental in chemistry education and research:
Example: Chemistry students conduct an experiment to verify Faraday's Law by electroplating copper. Using the calculator, they can predict the expected mass deposition and compare it with experimental results to calculate efficiency and identify sources of error.
Understanding electrolysis helps in designing corrosion protection systems:
Example: A marine engineering company designs cathodic protection for offshore platforms. The calculator helps determine the mass of sacrificial anodes needed and their expected lifetime based on the calculated rate of consumption.
Electrolysis is used in water treatment and hydrogen generation:
Example: A renewable energy company produces hydrogen through water electrolysis. The calculator helps them determine the production rate and efficiency of their electrolyzers, optimizing their operation for maximum hydrogen output.
While Faraday's Law provides a straightforward method for calculating electrolysis outcomes, there are alternative approaches and considerations:
For systems where reaction kinetics are important, the Butler-Volmer equation provides a more detailed model of electrode reactions, accounting for:
This approach is more complex but offers greater accuracy for systems with significant activation overpotential.
In industrial settings, empirical methods based on experimental data may be used:
These methods can account for real-world inefficiencies not captured by theoretical calculations.
Advanced computational methods provide comprehensive analysis:
These methods are particularly valuable for complex geometries and non-uniform current distributions.
The development of electrolysis as a scientific concept and industrial process spans several centuries, with Michael Faraday's work representing a pivotal moment in understanding the quantitative aspects of electrochemical reactions.
The foundation for electrolysis was laid in 1800 when Alessandro Volta invented the voltaic pile, the first electrical battery. This invention provided a continuous source of electricity, enabling new experiments:
These early experiments demonstrated the power of electricity to drive chemical reactions but lacked quantitative understanding.
Michael Faraday, who had been Davy's assistant, conducted systematic investigations into electrolysis in the 1830s. His meticulous experiments led to two fundamental laws:
Faraday's First Law of Electrolysis (1832): The mass of a substance altered at an electrode during electrolysis is directly proportional to the quantity of electricity transferred at that electrode.
Faraday's Second Law of Electrolysis (1834): For a given quantity of electricity, the mass of an elemental material altered at an electrode is directly proportional to the element's equivalent weight.
Faraday also introduced key terminology still used today:
Following Faraday's work, electrolysis rapidly developed industrial applications:
The 20th century saw refinements in understanding and applications:
Today, electrolysis remains a cornerstone of electrochemistry, with applications ranging from industrial-scale metal production to nanoscale material synthesis and energy storage technologies.
Here are implementations of Faraday's Law in various programming languages:
1' Excel formula for electrolysis calculation
2' Inputs in cells: A1=Current(A), B1=Time(s), C1=Molar Mass(g/mol), D1=Valency, E1=Faraday Constant
3=A1*B1*C1/(D1*E1)
4
5' Excel VBA function
6Function ElectrolysisCalculation(Current As Double, Time As Double, MolarMass As Double, Valency As Double) As Double
7 Dim FaradayConstant As Double
8 FaradayConstant = 96485
9 ElectrolysisCalculation = (Current * Time * MolarMass) / (Valency * FaradayConstant)
10End Function
111def calculate_electrolysis_mass(current, time, molar_mass, valency):
2 """
3 Calculate the mass of substance produced/consumed during electrolysis.
4
5 Parameters:
6 current (float): Current in amperes (A)
7 time (float): Time in seconds (s)
8 molar_mass (float): Molar mass in g/mol
9 valency (int): Valency number (electrons per ion)
10
11 Returns:
12 float: Mass in grams (g)
13 """
14 FARADAY_CONSTANT = 96485 # C/mol
15
16 # Apply Faraday's Law: m = (I * t * M) / (z * F)
17 mass = (current * time * molar_mass) / (valency * FARADAY_CONSTANT)
18
19 return mass
20
21# Example usage
22if __name__ == "__main__":
23 # Calculate copper deposition with 2A for 1 hour
24 copper_mass = calculate_electrolysis_mass(
25 current=2.0, # 2 amperes
26 time=3600, # 1 hour in seconds
27 molar_mass=63.55, # Copper molar mass in g/mol
28 valency=2 # Cu²⁺ valency
29 )
30
31 print(f"Mass of copper deposited: {copper_mass:.4f} grams")
321/**
2 * Calculate mass of substance produced/consumed during electrolysis
3 * @param {number} current - Current in amperes (A)
4 * @param {number} time - Time in seconds (s)
5 * @param {number} molarMass - Molar mass in g/mol
6 * @param {number} valency - Valency number (electrons per ion)
7 * @returns {number} Mass in grams (g)
8 */
9function calculateElectrolysisMass(current, time, molarMass, valency) {
10 const FARADAY_CONSTANT = 96485; // C/mol
11
12 // Apply Faraday's Law: m = (I * t * M) / (z * F)
13 const mass = (current * time * molarMass) / (valency * FARADAY_CONSTANT);
14
15 return mass;
16}
17
18// Example usage
19const materials = {
20 copper: { molarMass: 63.55, valency: 2, symbol: "Cu" },
21 silver: { molarMass: 107.87, valency: 1, symbol: "Ag" },
22 gold: { molarMass: 196.97, valency: 3, symbol: "Au" }
23};
24
25// Calculate silver deposition with 1.5A for 30 minutes
26const current = 1.5; // amperes
27const time = 30 * 60; // 30 minutes in seconds
28const material = materials.silver;
29
30const mass = calculateElectrolysisMass(
31 current,
32 time,
33 material.molarMass,
34 material.valency
35);
36
37console.log(`Mass of ${material.symbol} deposited: ${mass.toFixed(4)} grams`);
381public class ElectrolysisCalculator {
2 private static final double FARADAY_CONSTANT = 96485.0; // C/mol
3
4 /**
5 * Calculate mass of substance produced/consumed during electrolysis
6 *
7 * @param current Current in amperes (A)
8 * @param time Time in seconds (s)
9 * @param molarMass Molar mass in g/mol
10 * @param valency Valency number (electrons per ion)
11 * @return Mass in grams (g)
12 */
13 public static double calculateMass(double current, double time, double molarMass, int valency) {
14 // Apply Faraday's Law: m = (I * t * M) / (z * F)
15 return (current * time * molarMass) / (valency * FARADAY_CONSTANT);
16 }
17
18 public static void main(String[] args) {
19 // Calculate zinc deposition with 3A for 45 minutes
20 double current = 3.0; // amperes
21 double time = 45 * 60; // 45 minutes in seconds
22 double zincMolarMass = 65.38; // g/mol
23 int zincValency = 2; // Zn²⁺
24
25 double mass = calculateMass(current, time, zincMolarMass, zincValency);
26
27 System.out.printf("Mass of zinc deposited: %.4f grams%n", mass);
28 }
29}
301#include <iostream>
2#include <iomanip>
3
4/**
5 * Calculate mass of substance produced/consumed during electrolysis
6 *
7 * @param current Current in amperes (A)
8 * @param time Time in seconds (s)
9 * @param molarMass Molar mass in g/mol
10 * @param valency Valency number (electrons per ion)
11 * @return Mass in grams (g)
12 */
13double calculateElectrolysisMass(double current, double time, double molarMass, int valency) {
14 const double FARADAY_CONSTANT = 96485.0; // C/mol
15
16 // Apply Faraday's Law: m = (I * t * M) / (z * F)
17 return (current * time * molarMass) / (valency * FARADAY_CONSTANT);
18}
19
20int main() {
21 // Calculate nickel deposition with 2.5A for 2 hours
22 double current = 2.5; // amperes
23 double time = 2 * 3600; // 2 hours in seconds
24 double nickelMolarMass = 58.69; // g/mol
25 int nickelValency = 2; // Ni²⁺
26
27 double mass = calculateElectrolysisMass(current, time, nickelMolarMass, nickelValency);
28
29 std::cout << "Mass of nickel deposited: " << std::fixed << std::setprecision(4) << mass << " grams" << std::endl;
30
31 return 0;
32}
331using System;
2
3public class ElectrolysisCalculator
4{
5 private const double FaradayConstant = 96485.0; // C/mol
6
7 /// <summary>
8 /// Calculate mass of substance produced/consumed during electrolysis
9 /// </summary>
10 /// <param name="current">Current in amperes (A)</param>
11 /// <param name="time">Time in seconds (s)</param>
12 /// <param name="molarMass">Molar mass in g/mol</param>
13 /// <param name="valency">Valency number (electrons per ion)</param>
14 /// <returns>Mass in grams (g)</returns>
15 public static double CalculateMass(double current, double time, double molarMass, int valency)
16 {
17 // Apply Faraday's Law: m = (I * t * M) / (z * F)
18 return (current * time * molarMass) / (valency * FaradayConstant);
19 }
20
21 public static void Main()
22 {
23 // Calculate aluminum deposition with 5A for 3 hours
24 double current = 5.0; // amperes
25 double time = 3 * 3600; // 3 hours in seconds
26 double aluminumMolarMass = 26.98; // g/mol
27 int aluminumValency = 3; // Al³⁺
28
29 double mass = CalculateMass(current, time, aluminumMolarMass, aluminumValency);
30
31 Console.WriteLine($"Mass of aluminum deposited: {mass:F4} grams");
32 }
33}
34To calculate mass deposited in electrolysis, use Faraday's Law formula: m = (I × t × M) / (z × F), where I is current (amperes), t is time (seconds), M is molar mass (g/mol), z is valency, and F is Faraday's constant (96,485 C/mol). Simply input these values into our calculator for instant results.
The electrolysis mass calculation formula is m = (I × t × M) / (z × F). This formula, based on Faraday's Law, calculates the exact mass of substance produced or consumed during the electrochemical process.
Electrolysis is an electrochemical process that uses direct electric current (DC) to drive a non-spontaneous chemical reaction. It involves passing electricity through an electrolyte, causing chemical changes at the electrodes. During electrolysis, oxidation occurs at the anode (positive electrode) and reduction occurs at the cathode (negative electrode).
Faraday's Law establishes the quantitative relationship between the amount of electrical charge passed through an electrolyte and the amount of substance transformed at an electrode. It states that the mass of a substance produced at an electrode is directly proportional to the quantity of electricity transferred at that electrode and to the equivalent weight of the substance.
Several factors can affect electrolysis efficiency and mass deposition:
Our electrolysis calculator supports common metals including copper, silver, gold, zinc, nickel, iron, and aluminum. Each material has pre-configured molar mass and valency values. For other materials, you can manually apply the formula using the specific material's molar mass and valency number.
Electrolysis mass calculations using Faraday's Law provide theoretically perfect results assuming 100% current efficiency. In real-world applications, actual yield may be 90-98% due to side reactions, current leakage, or other inefficiencies. Our calculator gives the theoretical maximum mass deposition.
The calculator requires time input in seconds. To convert from other units:
The anode is the positive electrode where oxidation occurs (electrons are lost). The cathode is the negative electrode where reduction occurs (electrons are gained). In metal deposition, the metal ions in solution gain electrons at the cathode and are deposited as solid metal.
Faraday's Law provides theoretically perfect calculations assuming 100% current efficiency. In real-world applications, the actual yield may be lower due to side reactions, current leakage, or other inefficiencies. Industrial processes typically operate at 90-98% efficiency depending on conditions.
Yes, the same principles apply to batteries and fuel cells, which are essentially electrolysis in reverse. Faraday's Law can be used to calculate the theoretical capacity of a battery or the amount of reactant consumed in a fuel cell based on the current drawn.
Current efficiency is the percentage of the total current that goes toward the desired electrochemical reaction. It's calculated as the ratio of the actual mass deposited to the theoretical mass calculated from Faraday's Law, expressed as a percentage.
Temperature doesn't directly appear in Faraday's Law, but it can affect the efficiency of the electrolysis process. Higher temperatures generally increase reaction rates and reduce solution resistance, but may also increase side reactions. The calculator assumes standard conditions, so actual results may vary with temperature changes.
Faraday, M. (1834). "Experimental Researches in Electricity. Seventh Series." Philosophical Transactions of the Royal Society of London, 124, 77-122.
Bard, A. J., & Faulkner, L. R. (2000). Electrochemical Methods: Fundamentals and Applications (2nd ed.). John Wiley & Sons.
Pletcher, D., & Walsh, F. C. (1993). Industrial Electrochemistry (2nd ed.). Springer.
Schlesinger, M., & Paunovic, M. (2010). Modern Electroplating (5th ed.). John Wiley & Sons.
Hamann, C. H., Hamnett, A., & Vielstich, W. (2007). Electrochemistry (2nd ed.). Wiley-VCH.
Bockris, J. O'M., & Reddy, A. K. N. (1998). Modern Electrochemistry (2nd ed.). Plenum Press.
Lide, D. R. (Ed.). (2005). CRC Handbook of Chemistry and Physics (86th ed.). CRC Press.
Atkins, P., & de Paula, J. (2014). Atkins' Physical Chemistry (10th ed.). Oxford University Press.
Ready to calculate precise mass deposition for your electrolysis process? Try our free Electrolysis Calculator now to quickly determine the mass of material produced or consumed in your electrochemical applications. Simply enter your current, time, and select your electrode material to get instant, accurate results based on Faraday's Law.
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Meta Title: Electrolysis Calculator - Calculate Mass Deposition with Faraday's Law Meta Description: Calculate precise electrolysis mass deposition using Faraday's Law. Free online calculator for electroplating, metal refining, and electrochemistry applications.
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