======Aluminum and Copper(II) Chloride Redox Reaction======


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**Materials: **{{$demo.materials_description}}\\
**Difficulty: **{{$demo.difficulty_description}}\\
**Safety: **{{$demo.safety_description}}\\
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**Alternative titles:** Foiled Again
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====Summary====                   
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====Procedure====  
  - Add 0.5 M copper(II) chloride solution into a beaker.  
  - Cut a piece of aluminum foil and loosely crumple it so it will fit in the beaker.  
  - Place the foil into the solution, using a stirring rod to submerge it fully.  
  - Observe the reaction: bubbling gas, strong heating, fading of the green-blue solution, and formation of reddish-brown copper metal.  
  - Test the gas released with a lit splint (hydrogen gives a “pop”) or with a glowing splint (no re-ignition; confirms no oxygen).  
  - Compare with control tests by placing aluminum foil into copper(II) sulfate solution (no reaction), sodium chloride solution (no reaction), or both together (reaction occurs due to chloride complexation).  
  - Allow the solid copper to settle and decant the liquid for safe disposal.  




====Links==== 
Foiled Again - FlinnScientific: 
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Aluminum and Copper (II) Chloride Reaction - Bond with James: 
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📄 Foiled Again — Aluminum Loses
to Copper - Flinn Scientific: [[https://www.flinnsci.ca/api/library/Download/7202c51528a240ec81e731e2142c53c4]]\\


====Variations====
  * Try using different shapes or surface areas of aluminum foil to see how reaction rate changes.

====Safety Precautions====
  * Wear chemical splash goggles, chemical-resistant gloves, and a protective apron.  
  * Copper(II) chloride is toxic; avoid ingestion and skin contact.  
  * The reaction produces hydrogen gas, which is highly flammable; keep flames away and perform in a well-ventilated area.  
  * The reaction is exothermic; the beaker may become hot to touch. Handle with care.  
  * Dispose of solutions and solids according to hazardous waste guidelines; do not pour copper solutions directly down the drain unless allowed by local regulations.




====Questions to Consider====
  * Write the balanced equation for the main reaction. (2Al + 3CuCl₂ → 2AlCl₃ + 3Cu)  
  * Which element is oxidized and which is reduced? (Aluminum is oxidized to Al³⁺; copper(II) is reduced to Cu metal)  
  * Why does hydrogen gas form as a side reaction? (Because the solution is slightly acidic, allowing H⁺ ions to react with aluminum)  
  * How does the surface area of the aluminum foil affect the rate of reaction? (Greater surface area increases reaction rate)  
  * Why does aluminum not react with copper(II) sulfate alone? (Chloride ions are needed to break through aluminum’s oxide layer and catalyze the reaction)