AScholarix Academy

Chemistry · Mission: Power the City

Electrochemistry

Become an electrochemical engineer. Restore power by building a battery, understanding electron movement, calculating voltage, running electrolysis and protecting iron from rust.

🎯 Electron transfer drives redox reactions, galvanic cells convert chemical energy into electrical energy, electrolysis uses electricity to drive chemical change, and corrosion is an electrochemical process that we can control.

⚡ Your guide: Engineer Maya, electrochemical engineer. · Source: Plus Two Chemistry · step-by-step video storyboard (12-page lesson storyboard)

Start Level 1: Electron Energy Lab →Mentor

Levels

0/7

XP

0

Rank

Trainee

Streak

0 days

Mastered

0/18

Final

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Mission map

  1. 1Level 1Electron Energy LabOxidation, reduction and redox3 scenes
  2. 🔒Level 2Build a BatteryGalvanic cell and electron flowPass Level 1 to unlock
  3. 🔒Level 3Cell Notation GateAnode, cathode and salt bridgePass Level 2 to unlock
  4. 🔒Level 4Voltage Control RoomElectrode potential and EMFPass Level 3 to unlock
  5. 🔒Level 5Nernst ChallengeConcentration and cell potentialPass Level 4 to unlock
  6. 🔒Level 6Electrolysis FactoryFaraday's laws and calculationsPass Level 5 to unlock
  7. 🔒Level 7Rust RescueCorrosion and preventionPass Level 6 to unlock
Virtual Lab18 hands-on experiments with live apparatus, a lab notebook and Engineer Maya's voice. 0/18 done.Enter the lab →Problem sets48 problems across 7 levels: 🌍 real life · 📝 exam style · 💡 understanding · 🛠️ applied.Solve problems →

Practice & assessment

🧭

Guided practice

Questions from levels you've unlocked, with hints.

🎯

Independent practice

No hints, plus fresh engine-generated questions. Proves mastery.

🔁

Revision practice

Targets your weak concepts and past mistakes.

🗣️

Oral revision

Explain ideas out loud to your teacher.

🏁

Final assessment

The end-of-course test. 70% to pass.

⚡

Challenge mode

Harder mixed questions, no hints. Beat your best.

Badges

🕵️Electron Detective🔋Battery Builder🗝️Gate Keeper🎛️Voltage Controller📉Nernst Navigator🏭Factory Chief🌆City Restored🔮Sharp Predictor🔥Three-Day Streak🧠Concept Master🎓Course Complete

Concept mastery

Mastery needs repeated correct answers including at least one without help — finishing a lesson alone doesn’t count.

  • Oxidation (loss of electrons)not started
  • Reduction (gain of electrons)not started
  • Redox and agentsnot started
  • Anode (zinc, oxidation)not started
  • Cathode (copper, reduction)not started
  • Salt bridge and ion movementnot started
  • Cell notationnot started
  • Electrode potentialnot started
  • Standard hydrogen electrodenot started
  • EMF calculationnot started
  • Nernst equationnot started
  • Reaction quotient Qnot started
  • Electrolytic vs galvanic cellsnot started
  • Faraday's first lawnot started
  • Faraday mass calculationnot started
  • Faraday's second lawnot started
  • Corrosionnot started
  • Rust preventionnot started
Glossary
+
— Plus: added to / together with.
→
— Forms / produces: the reaction proceeds in the shown direction.
e⁻
— Electron: a negatively charged particle.
²⁺
— Two plus: positive charge of two.
⁻
— Minus: negative charge of one.
(s)
— Solid: substance is a solid.
(aq)
— Aqueous: dissolved in water.
|
— Phase boundary: boundary between phases in cell notation.
||
— Salt bridge: boundary representing the salt bridge.
E°
— E naught: standard electrode or cell potential.
log
— Logarithm: here, common logarithm with base 10.
∝
— Proportional to: if one doubles, the other doubles under the stated conditions.
Q
— Charge or reaction quotient: charge in electrolysis; reaction quotient in Nernst.
I
— Current: flow of electric charge, measured in amperes.
t
— Time: duration, measured in seconds in the calculation.
F
— Faraday constant: approximately 96,485 coulombs per mole.
M
— Molar mass: mass of one mole of a substance.
n
— Electron number: number of electrons in the balanced electrode reaction.
Accuracy notes
  • Never show a numerical formula before explaining the physical event.
  • In calculations, reveal substitution one line at a time and keep units visible.
  • Q means charge in electrolysis and the reaction quotient in the Nernst equation.
  • Faraday calculations assume 100% current efficiency; real processes may deposit less because of side reactions.
  • In precise thermodynamics, activities are used; concentrations are an approximation in suitable dilute solutions.
  • Electrode potentials other than Cu (+0.34 V) and Zn (−0.76 V) are NCERT table values used as extensions.
Optional extensions
  • More electrode pairs. The cell builder includes Mg, Al, Fe, Ni, Pb and Ag with NCERT standard reduction potentials.
  • Temperature in the Nernst equation. E = E° − (2.303RT/nF) log Q; at 298 K the factor 2.303RT/F ≈ 0.0591 V.
  • Salt and corrosion. Dissolved salt makes water a better electrolyte and speeds up rusting (shown as an option in the corrosion lab).