Select plating metal, current density, area, and processing time to calculate film thickness, deposited mass, power consumption, and charge using Faraday's law in real time. Supports Ni, Cu, Cr, Au, and Zn.
Plating Metal
Ni: η=97%, M=58.7g/mol, n=2
Process Conditions
A/dm²
dm²
min
%
Results
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Coating Thickness δ (μm)
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Deposited Mass m (g)
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Electric Charge Q (C)
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Energy Use P (Wh)
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Thickness Rate (μm/min)
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Power Cost
Thickness
Processing time t and coating thickness δ have a linear relationship. Current density, current efficiency, and area use the current settings.
Current Efficiency
Shows how coating thickness changes with current efficiency η (10-100%). All other conditions are held constant.
Metal Comparison
Compares coating thickness and deposited mass for each metal under the same conditions (J=3 A/dm², t=30 min).
Theory & Key Formulas
Deposited mass \(m\) (g) when current \(I\) (A) flows for time \(t\) (s):
Where \(J = I/A\) (current density, A/m²) and \(\rho\) = density (kg/m³). This shows that \(\delta\) is proportional to \(J \cdot t\).
How Electroplating Works — A Conversational Guide
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In electroplating, when you pass an electric current, metal deposits on the surface, right? Why does that happen?
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It's an electrochemical reaction. Metal ions are dissolved in the plating solution (electrolyte). When you apply a current to the cathode (the part to be plated), these metal ions receive electrons (reduction reaction) and deposit as solid metal on the surface. For example, in nickel plating, the reaction is Ni²⁺ + 2e⁻ → Ni.
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What does it mean to use 'Faraday's law'?
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Faraday's law of electrolysis states that 'the amount of substance deposited is proportional to the amount of electricity passed.' The formula is m = M × Q / (n × F). M is the atomic mass, Q is the electric charge (coulombs), n is the ion valence (2 for Ni²⁺), and F = 96485 C/mol is Faraday's constant. Since Q = I × t (current × time), multiplying current and time gives the deposited mass.
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The current efficiency of chromium plating is 20–35%, which seems really low, doesn't it? Nearly 90% is wasted?
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Yes, chromium plating is special. In hexavalent chromium solutions, a large amount of hydrogen is generated, and most of the power is consumed by the hydrogen evolution reaction. That's why the plating voltage is high and power consumption is large. It also has a high environmental load, so switching to trivalent chromium plating or developing alternative technologies is progressing. For gold (Au), the current efficiency is very high at 95–99%.
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If you increase the current density, you can plate faster, right? So why is there an appropriate current density range?
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If the current density is too high, 'burning' occurs. When the deposition rate exceeds the supply rate of metal ions to the cathode surface, the ion concentration near the surface becomes depleted, resulting in a rough, grainy coating. Conversely, if it's too low, the deposition rate slows down, and smut (soot-like deposits) may occur. The appropriate range varies depending on the plating solution type, temperature, and agitation.
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What conditions are used for copper plating on printed circuit boards?
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For copper sulfate plating solution, J = 1–5 A/dm², and the target thickness is usually 15–30 μm (IPC standard). It's difficult to deposit uniformly inside vias (holes), so a 'slow current density' is used for gradual deposition, or pulse current (forward/reverse) is applied. With this tool, you can confirm that at J = 2 A/dm², η = 98%, and t = 30 minutes, the thickness is about 20 μm.
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Gold plating is often used in electronic components, but why use such expensive gold?
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Gold has properties essential for electronic components: it does not corrode, has low contact resistance, and offers good solderability. However, the thickness is often thin, around 0.05–1 μm. For connector sliding contacts, 0.5–1 μm is used for wear resistance; for bonding wire pads, about 0.3–0.5 μm. Comparing gold under the same conditions with this tool, since its atomic mass is 197 and valence is 1, you can see that the deposition rate is faster than copper.
Frequently Asked Questions
Deposited mass m = η × M × I × t / (n × F), then thickness δ = m / (ρ × A). M is atomic mass, I is current, t is time (seconds), n is ion valence, F is Faraday constant 96485 C/mol, ρ is density, A is plating area. Example: Ni (M=58.7, n=2, ρ=8.9 g/cm³) with I=15 A, t=1800 s, η=97%, A=5 dm² → δ ≈ 20 μm.
Low current efficiency (especially for Cr at 20–40%) increases power consumption and risks hydrogen embrittlement due to hydrogen gas incorporation into the coating. Post-plating baking (dehydrogenation at 190–220°C for several hours) is mandatory for high-strength steel. Proper ventilation is also critical to manage hydrogen gas in the workplace.
Hard chromium targets thicknesses of 20–500 μm for wear and heat resistance (HV 800–1000), used in cylinders, dies, and rolls. Decorative chromium targets 0.1–0.5 μm for gloss and corrosion resistance, requiring a Cu/Ni underlayer. Hard chromium uses current density 30–70 A/dm², decorative uses 10–20 A/dm² — significantly different.
Optimizing anode–cathode distance, enhancing agitation, controlling electrolyte concentration, and using edge effect countermeasures (e.g., shielding plates) are effective. For deep holes and complex shapes, pulse plating (forward/reverse) improves uniformity. Additives (brighteners, leveling agents) also play a key role in improving throwing power.
Hexavalent chromium (Cr⁶⁺) achieves glossy coatings with current efficiency of 20–35%, but is highly carcinogenic and toxic, subject to RoHS restrictions. Trivalent chromium (Cr³⁺) offers higher current efficiency (60–70%) and lower environmental impact, but thick coatings (>10 μm) are difficult and color tone differs slightly. Industry is rapidly transitioning to trivalent chromium.
Non-uniform current density distribution directly leads to uneven thickness, so FEM (finite element method) analysis of primary and secondary current distributions is performed. In Abaqus or COMSOL, the Laplace equation (∇²φ=0) is solved to predict potential distribution → current density → thickness distribution. CAE is practically applied to optimize plating uniformity for complex shapes like dies and connectors.
What is Electroplating?
Electroplating is a fundamental topic in engineering and applied physics. This interactive simulator lets you explore the key behaviors and relationships by directly manipulating parameters and observing real-time results.
By combining numerical computation with visual feedback, the simulator bridges the gap between abstract theory and physical intuition — making it an effective learning tool for students and a rapid-verification tool for practicing engineers.
Physical Model & Key Equations
The simulator is based on the governing equations behind Electroplating Thickness Calculator. Understanding these equations is key to interpreting the results correctly.
Each parameter in the equations corresponds to a slider in the control panel. Moving a slider changes the equation's solution in real time, helping you build a direct connection between mathematical expressions and physical behavior.
Real-World Applications
Engineering Design: The concepts behind Electroplating Thickness Calculator are applied across mechanical, structural, electrical, and fluid engineering disciplines. This tool provides a quick way to estimate design parameters and sensitivity before committing to full CAE analysis.
Education & Research: Widely used in engineering curricula to connect theory with numerical computation. Also serves as a first-pass validation tool in research settings.
CAE Workflow Integration: Before running finite element (FEM) or computational fluid dynamics (CFD) simulations, engineers use simplified models like this to establish physical scale, identify dominant parameters, and define realistic boundary conditions.
Common Misconceptions and Points of Caution
Model assumptions: The mathematical model used here relies on simplifying assumptions such as linearity, homogeneity, and isotropy. Always verify that your real system satisfies these assumptions before applying results directly to design decisions.
Units and scale: Many calculation errors arise from unit conversion mistakes or order-of-magnitude errors. Pay close attention to the units shown next to each parameter input.
Validating results: Always sanity-check simulator output against physical intuition or hand calculations. If a result seems unexpected, review your input parameters or verify with an independent method.
Select metal type (copper, nickel, zinc, chromium) from the dropdown to set atomic mass and valence electrons
Enter current density in A/dm² using the slider or numeric input (typical range 1–10 A/dm²)
Input plating area in dm² (convert your workpiece size: 100 cm² = 1 dm²)
Set plating time in minutes; the simulator calculates deposit thickness via Faraday's law: thickness = (I·t·M)/(n·F·ρ·A)
View results: coating thickness in micrometers, deposited mass in grams, and power consumption in watts
Worked Example
Copper plating on a steel connector: current density 5 A/dm², area 2 dm², plating time 30 minutes. Using Faraday's law with M=63.5 g/mol, n=2 valence, F=96485 C/mol, ρ=8.96 g/cm³, the calculator yields approximately 75 micrometers thickness, 13.5 g deposited copper, and 180 W average power consumption (assuming 5 V cell voltage). Verify against industrial specs: automotive contacts typically require 10–50 μm copper strike layers.
Practical Notes
Current density affects plating uniformity and deposit quality; exceed 8 A/dm² on zinc to risk dendrite formation and poor adhesion on recessed features
Area calculation must include all surfaces; blind holes and internal geometries reduce effective cathode area by 20–40%
Power consumption scales linearly with time and current; a 10 A/dm² copper plating bath at 6 V consumes ~60 W/dm² and generates significant heat—use cooling systems above 30 minute runs
Chromium plating requires trivalent (Cr³⁺) baths for better efficiency than hexavalent routes; adjust valence accordingly in the dropdown