{"success":true,"version":"v1","request":{"tool":"get_calculator_schema","calculator_id":"faraday-electrolysis"},"result":{"entity_type":"calculator","id":"faraday-electrolysis","calculator_id":"faraday-electrolysis","canonical_url":"https://tttkmbb.com/chemistry/faraday-electrolysis","name":"Faraday's Law of Electrolysis Calculator","title":"Electrolysis Calculator – Mass Deposited, Charge and Moles of Electrons from Current and Time (Faraday's Laws)","category":"chemistry","category_name":"Chemistry","tool_name":"calculate_faraday_electrolysis","featured_mcp_tool":false,"description":"Applies Faraday's laws of electrolysis: from current and time it computes the charge passed, moles of electrons, moles and mass of substance deposited or evolved (m = Q·M / (z·F)), or, for a target mass, the electrolysis time required at the given current.","use_when":"You need how much metal is plated or gas is evolved by a current over a time, or how long an electrolysis must run at a given current to produce a target mass.","do_not_use_when":"The current efficiency is well below 100% (side reactions such as hydrogen evolution reduce the real yield), or you need the cell voltage rather than the amount of product (use nernst-equation).","inputs":[{"name":"current_a","label":"Current","type":"number","unit":"A","required":true,"exclusive_min":0,"description":"Constant electrolysis current in amperes.","example":10.23},{"name":"time","label":"Time","type":"number","required":false,"exclusive_min":0,"description":"Duration of electrolysis in time_unit. Leave empty to solve it from target_mass_g.","example":1},{"name":"time_unit","label":"Time unit","type":"enum","required":false,"default":"seconds","values":[{"value":"seconds","label":"seconds","aliases":["s","sec"]},{"value":"minutes","label":"minutes","aliases":["min","m"]},{"value":"hours","label":"hours","aliases":["h","hr"]}],"description":"Unit of the time input.","example":"hours"},{"name":"electrons_per_ion","label":"Electrons per atom or molecule z","type":"integer","required":true,"min":1,"max":12,"description":"Moles of electrons per mole of product: Ag⁺ → Ag 1, Cu²⁺ → Cu 2, Al³⁺ → Al 3, 2H⁺ → H2 2, 2H2O → O2 4, 2Cl⁻ → Cl2 2.","example":1},{"name":"formula","label":"Chemical formula","type":"string","required":false,"description":"Formula of the substance deposited or evolved (Ag, Cu, Al, H2, O2, Cl2) for its molar mass. Alternative to molar_mass_g_mol.","example":"Ag"},{"name":"molar_mass_g_mol","label":"Molar mass","type":"number","unit":"g/mol","required":false,"max":10000000,"exclusive_min":0,"description":"Molar mass of the substance; use instead of formula when it is already known."},{"name":"target_mass_g","label":"Target mass","type":"number","unit":"g","required":false,"exclusive_min":0,"description":"Mass of product wanted; when given, the calculator solves the time needed at current_a (the time input is ignored)."}],"outputs":[{"name":"charge_c","label":"Charge passed","type":"number","unit":"C","decimals":3,"description":"Q = I × t."},{"name":"moles_electrons","label":"Moles of electrons","type":"number","unit":"mol","decimals":6,"description":"Q / F (F = 96 485.33 C/mol)."},{"name":"moles_substance","label":"Moles of product","type":"number","unit":"mol","decimals":6,"description":"moles_electrons / z."},{"name":"mass_g","label":"Mass of product","type":"number","unit":"g","decimals":4,"description":"moles_substance × molar mass."},{"name":"gas_volume_stp_l","label":"Volume if a gas (0 °C, 1 atm)","type":"number","unit":"L","decimals":4,"description":"moles_substance × 22.414 L/mol; meaningful only for gaseous products such as H2, O2 or Cl2."},{"name":"time_s","label":"Time","type":"number","unit":"s","decimals":3,"description":"Electrolysis time in seconds."},{"name":"time_min","label":"Time","type":"number","unit":"min","decimals":4,"description":"Electrolysis time in minutes."},{"name":"time_h","label":"Time","type":"number","unit":"h","decimals":5,"description":"Electrolysis time in hours."},{"name":"molar_mass_g_mol","label":"Molar mass","type":"number","unit":"g/mol","decimals":3,"description":"Molar mass of the product used."},{"name":"solved_for","label":"Solved for","type":"string","decimals":4,"description":"mass_g (from current and time) or time_s (from target mass)."}],"input_schema":{"type":"object","properties":{"current_a":{"description":"Constant electrolysis current in amperes. Unit: A.","type":"number","exclusiveMinimum":0,"examples":[10.23],"x-unit":"A"},"time":{"description":"Duration of electrolysis in time_unit. Leave empty to solve it from target_mass_g.","type":"number","exclusiveMinimum":0,"examples":[1]},"time_unit":{"description":"Unit of the time input.","type":"string","enum":["seconds","minutes","hours"],"default":"seconds","examples":["hours"]},"electrons_per_ion":{"description":"Moles of electrons per mole of product: Ag⁺ → Ag 1, Cu²⁺ → Cu 2, Al³⁺ → Al 3, 2H⁺ → H2 2, 2H2O → O2 4, 2Cl⁻ → Cl2 2.","type":"integer","minimum":1,"maximum":12,"examples":[1]},"formula":{"description":"Formula of the substance deposited or evolved (Ag, Cu, Al, H2, O2, Cl2) for its molar mass. Alternative to molar_mass_g_mol.","type":"string","examples":["Ag"]},"molar_mass_g_mol":{"description":"Molar mass of the substance; use instead of formula when it is already known. Unit: g/mol.","type":"number","maximum":10000000,"exclusiveMinimum":0,"x-unit":"g/mol"},"target_mass_g":{"description":"Mass of product wanted; when given, the calculator solves the time needed at current_a (the time input is ignored). Unit: g.","type":"number","exclusiveMinimum":0,"x-unit":"g"}},"additionalProperties":false,"required":["current_a","electrons_per_ion"]},"output_schema":{"type":"object","properties":{"charge_c":{"description":"Q = I × t. Unit: C.","type":"number","x-unit":"C"},"moles_electrons":{"description":"Q / F (F = 96 485.33 C/mol). Unit: mol.","type":"number","x-unit":"mol"},"moles_substance":{"description":"moles_electrons / z. Unit: mol.","type":"number","x-unit":"mol"},"mass_g":{"description":"moles_substance × molar mass. Unit: g.","type":"number","x-unit":"g"},"gas_volume_stp_l":{"description":"moles_substance × 22.414 L/mol; meaningful only for gaseous products such as H2, O2 or Cl2. 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Unit: g/mol.","type":"number","x-unit":"g/mol"},"solved_for":{"description":"mass_g (from current and time) or time_s (from target mass).","type":"string"}}},"formula":"Q = I × t; n_e = Q / F; n = n_e / z; m = n × M = I × t × M / (z × F) with F = 96485.33212 C/mol; time for a target mass: t = m × z × F / (M × I)","method":"Assumes 100% current efficiency (all charge goes into the stated product) and a constant current; real plating baths typically run at 90–98% efficiency.","sources":[{"name":"OpenStax Chemistry 2e – 17.7 Electrolysis","url":"https://openstax.org/books/chemistry-2e/pages/17-7-electrolysis","type":"textbook","retrieved_at":"2026-09-24"},{"name":"Wikipedia – Faraday's laws of electrolysis","url":"https://en.wikipedia.org/wiki/Faraday%27s_laws_of_electrolysis","type":"reference","retrieved_at":"2026-09-24"},{"name":"NIST – CODATA internationally recommended values of the fundamental physical constants (Faraday constant F = 96 485.33212 C/mol, exact)","url":"https://physics.nist.gov/cuu/Constants/index.html","type":"standard","retrieved_at":"2026-09-24"}],"freshness":{"type":"static","max_age_seconds":null,"note":"Deterministic formula with fixed constants; results never go stale. Inputs supplied by the caller determine the output."},"examples":[{"name":"Silver plating at 10.23 A for 1 hour","inputs":{"current_a":10.23,"time":1,"time_unit":"hours","electrons_per_ion":1,"formula":"Ag"},"expected":{"charge_c":36828,"moles_electrons":0.381695,"moles_substance":0.381695,"mass_g":41.1735,"time_s":3600,"molar_mass_g_mol":107.87,"solved_for":"mass_g"},"url":"https://tttkmbb.com/api/v1/calculate/faraday-electrolysis?current_a=10.23&time=1&time_unit=hours&electrons_per_ion=1&formula=Ag"},{"name":"Time to deposit 10.0 g of copper at 5.0 A","inputs":{"current_a":5,"electrons_per_ion":2,"formula":"Cu","target_mass_g":10},"expected":{"moles_substance":0.157366,"moles_electrons":0.314733,"charge_c":30367.08,"time_s":6073.42,"time_min":101.224,"time_h":1.68706,"solved_for":"time_s"},"url":"https://tttkmbb.com/api/v1/calculate/faraday-electrolysis?current_a=5&electrons_per_ion=2&formula=Cu&target_mass_g=10"}],"faq":[{"q":"How do I choose z?","a":"z is the number of electrons per atom or molecule of product in the half-reaction: the ion charge for metals (Cu²⁺ + 2e⁻ → Cu gives 2), 2 for H2 or Cl2, 4 for O2 from water."},{"q":"What if the current is not constant?","a":"Use the total charge instead: enter the average current and the total time, since Q = ∫I dt; a coulometer reading divided by any time gives the equivalent constant current."}],"tags":["faraday's law","electrolysis","electroplating","mass deposited","coulombs","moles of electrons"],"related":[{"calculator_id":"moles-mass","reason":"Convert the moles of product to atoms or check the mass."},{"calculator_id":"nernst-equation","reason":"Cell potential of the same electrochemical reaction."},{"calculator_id":"electric-power","reason":"Energy consumed from current, voltage and time."}],"links":{"html":"https://tttkmbb.com/chemistry/faraday-electrolysis","markdown":"https://tttkmbb.com/chemistry/faraday-electrolysis.md","json":"https://tttkmbb.com/chemistry/faraday-electrolysis.json","api":"https://tttkmbb.com/api/v1/calculate/faraday-electrolysis","schema":"https://tttkmbb.com/api/v1/calculators/faraday-electrolysis","openapi":"https://tttkmbb.com/openapi.json","mcp":"https://tttkmbb.com/mcp"},"version":"v1","updated_at":"2026-09-24"},"timestamp":"2026-09-24T01:48:12Z"}