Chemistry Lab from Chemistry Code

electrochemical systems, batteries, and organic laboratory preparations with realistic apparatus design

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Galvanic (Voltaic) Cells
Spontaneous redox reactions producing electrical energy
Daniell Cell Primary · Galvanic
V 1.10 V e⁻ → SALT BRIDGE Na₂SO₄ SO₄²⁻ Na⁺ Zn mass ↓ Zn²⁺ Zn²⁺ Zn²⁺ ANODE (−) ZnSO₄(aq) Zn → Zn²⁺ + 2e⁻ (Oxidation) Cu mass ↑ Cu²⁺ Cu²⁺ CATHODE (+) CuSO₄(aq) Cu²⁺ + 2e⁻ → Cu (Reduction)
⚛ Anodic Reaction (Oxidation)
Zn(s) → Zn²⁺(aq) + 2e⁻
E° = +0.76 V
Standard Hydrogen Electrode(SHE) Reference · E° = 0.00 V
H₂ 1 atm H₂ Tank Pt(s) Platinized HCl(aq) · [H⁺] = 1 M Glass jacket
⚛ Anodic Reaction (Oxidation)
H₂(g) → 2H⁺(aq) + 2e⁻
Reference standard, E° = 0.00 V
Mercury Cell Primary · Compact
Zn(Hg) AMALGAM ANODE KOH-saturated separator + ZnO HgO + GRAPHITE CATHODE − + 💡 Powered Device
⚛ Anodic Reaction (Oxidation)
Zn(S) + 2OH⁻ → ZnO(s) + H₂O + 2e⁻
Fuel Cell (Hydrogen-Oxygen cell) Continuous · Green Energy
KOH Electrolyte OH⁻ OH⁻ H₂ → Hydrogen fuel Excess H₂ ← ← O₂ Oxygen H₂O → M ANODE (−) CATHODE (+)
⚛ Anodic Reaction (Oxidation)
2H₂(g) + 4OH⁻ → 4H₂O(l) + 4e⁻
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Rechargeable Batteries
Secondary cells - reversible electrochemical energy storage
Lead-Acid Car Battery(Lead accumulator) 12V · 6 Cells · Secondary
Cell 1 Cell 2 Cell 3 Cell 4 Cell 5 Cell 6 − + Pb (anode) PbO₂ (cathode) 6 × 2.05V = 12V H⁺ SO₄²⁻ Dilute H₂SO₄ Electrolyte Pb+SO₄²⁻→PbSO₄+2e⁻ PbO₂+4H⁺+SO₄²⁻+2e⁻→PbSO₄+2H₂O e⁻ (discharge →)
⚛ Anodic Reaction (Discharge)
Pb(s) + SO₄²⁻ → PbSO₄(s) + 2e⁻
Lithium-Ion Battery 3V · Secondary
+ − Li-ION 18650 Cu LiC₆ (Anode) LiPF₆ in organic solvent Li⁺ migration LiCoO₂ (Cathode) Al e⁻ (Discharge) ANODE (−) CATHODE (+)
⚛ Anodic Reaction (Discharge)
LiC₆ → C₆ + Li⁺ + e⁻
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Electrolytic Cells
Non-spontaneous reactions driven by external electrical energy
Electrolysis of CuCl₂ Solution Decomposition
6.00 V ON DC POWER + − ANODE (+) Cl₂↑ CATHODE (−) Cu deposit Cu²⁺ Cu²⁺ Cl⁻ Cl⁻ CuCl₂(aq)
⚛ Anodic Reaction (Oxidation)
2Cl⁻(aq) → Cl₂(g) + 2e⁻
Extraction Process of Al Industrial · 950°C
Steel shell Carbon lining (cathode) ⬇ MOLTEN ALUMINUM ⬇ Al₂O₃ dissolved in Cryolite (Na₃AlF₆) ~950°C molten electrolyte CARBON ANODES (+) CO₂↑ Al tap DC
⚛ Anodic Reaction (Oxidation)
6O²⁻ → 3/2O₂(g) + 6e⁻
Silver Electroplating Surface Coating
− + BATTERY CATHODE (−) Spoon Ag ANODE (+) Pure Silver Ag⁺ Ag⁺ Ag⁺ AgNO₃(aq) Solution
⚛ Anodic Reaction (Oxidation)
Ag(s) → Ag⁺(aq) + e⁻
Electrolytic Copper Refining 99.99% Purity
DC Supply ~0.3 V (low) − + CATHODE (−) Pure Cu (thin) ANODE (+) Impure Cu Anode mud(sludge) (Au, Ag, Pt) Cu²⁺ Cu²⁺ Acidified CuSO₄(aq)
⚛ Anodic Reaction (Oxidation)
Cu(impure) → Cu²⁺(aq) + 2e⁻
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Organic Lab Preparations
Laboratory synthesis of important hydrocarbons
Preparation of Methane(dry distillation) Decarboxylation · CH₄
CH₃COONa+CaO OPEN CH₄ methane
🧪 Decarboxylation (Soda-Lime)
CH₃COONa + NaOH ━(CaO/Δ)→ CH₄↑ + Na₂CO₃
Collect over water · methane is insoluble
Preparation of Ethylene(Dehydration) Dehydration · C₂H₄
180°C Ethanol + Conc. H₂SO₄ NaOH wash OPEN C₂H₄ ethylene
🧪 Dehydration of Ethanol
C₂H₅OH ━(Conc.H₂SO₄/180°C)→ C₂H₄↑ + H₂O
NaOH removes acidic impurities (SO₂, CO₂)
Preparation of Acetylene(water dripping) Hydrolysis · C₂H₂
H₂O CaC₂ chunks CuSO₄ +H₂SO₄ remove H₂S, PH₃ OPEN C₂H₂ acetylene
🧪 Hydrolysis of Calcium Carbide
CaC₂ + 2H₂O → C₂H₂↑ + Ca(OH)₂
CuSO₄+H₂SO₄ wash removes H₂S, PH₃ impurities
Test for hydrogen and hydrogen in Organic Compounds (C & H) Combustion Test
Org+CuO CuSO₄ H₂O Lime Water Ca(OH)₂ turns milky → CO₂ present
🧪 Hydrogen Detection
H₂ + CuO ━Δ→ Cu + H₂O
Water turns anhydrous white CuSO₄ → blue (CuSO₄·5H₂O)
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