#electrochemistry

Faraday-law electrolysis maths as an API, computed locally and deterministically. The mass endpoint applies Faraday's first law of electrolysis, m = (Q·M)/(n·F) = (I·t·M)/(n·F), to give the mass of a substance deposited at a cathode or dissolved at an anode from the charge passed — or the current and time — the molar mass and the valence (electrons transferred per ion), with the Faraday constant 96485 C/mol. The charge endpoint inverts it to give the charge Q = (m·n·F)/M and, with a current, the plating time needed to deposit a target mass — the core sizing calculation for electroplating and anodising. The gas-volume endpoint computes the volume of gas evolved during electrolysis, moles = Q/(n·F) and volume = moles × 22.414 L/mol at STP, using the electrons per gas molecule (two for hydrogen, four for oxygen in water electrolysis). Molar mass is in g/mol, current in amperes, time in seconds, charge in coulombs and mass in grams. Everything is computed locally and deterministically, so it is instant and private. Ideal for electroplating, anodising, battery, hydrogen-production and chemistry-education app developers, plating-time and gas-yield tools, and electrochemistry teaching. Pure local computation — no key, no third-party service, instant. Live, nothing stored. 3 endpoints. This is electrolysis (Faraday's laws); for cell potential and the Nernst equation use an electrochemistry Nernst API.

api.oanor.com/electrolysis-api

Electrochemistry maths as an API, computed locally and deterministically. The nernst endpoint applies the Nernst equation, E = E° − (R·T/nF)·ln Q, to give the actual electrode or cell potential under non-standard conditions from the standard potential E°, the number of electrons transferred n, the reaction quotient Q and the temperature — at 25 °C this reduces to E = E° − (0.05916/n)·log10 Q, and a larger Q (more product) lowers the potential. The cell-potential endpoint computes a galvanic cell's standard EMF from the cathode and anode standard reduction potentials, E°cell = E°cathode − E°anode, together with the standard Gibbs free energy ΔG° = −nF·E°cell and whether the reaction is spontaneous. The equilibrium endpoint computes the equilibrium constant of a redox reaction, K = exp(nF·E°cell / RT), and the corresponding ΔG°, from the standard cell potential and the electrons transferred. Potentials are in volts, energies in kJ/mol, the Faraday constant is 96485 C/mol and the gas constant 8.314 J/mol·K. Everything is computed locally and deterministically, so it is instant and private. Ideal for chemistry-education, battery, corrosion, electroplating and electroanalytical app developers, galvanic-cell and redox tools, and STEM teaching. Pure local computation — no key, no third-party service, instant. Live, nothing stored. 3 endpoints. This is electrochemistry; for acid-base pH use a pH API and for reaction-rate kinetics an Arrhenius API.

api.oanor.com/nernst-api