======Can Ripper======


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**Difficulty: **{{$demo.difficulty_description}}\\
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**Alternative titles:** Carving a Can with Chemistry, Aluminium vs Copper Chloride
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====Summary====                   
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====Procedure====  
 - Use a triangular file to carefully score a fine line around the inside of an empty soda can, about halfway down. This exposes the aluminum beneath the protective coating.  
  - Dissolve about 10 g of copper(II) chloride in 200 mL of warm water. Pour this solution into the can so it covers the scored area.  
  - Allow the can to sit for 3–5 minutes until the reaction is complete. The aluminum will dissolve along the scored line, visible as darkening paint on the outside.  
  - Carefully pour out the solution and rinse the can with water.  
  - Hold the can with both hands on either side of the scoring and twist firmly. The can should rip apart along the weakened line.



====Links==== 
Ripping a can in half using science - Imagination Station Toledo: 
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Can Ripper - Flinn Scientific: 
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📄 Can Ripper - Flinn Scientific: [[https://www.flinnsci.com/api/library/Download/0c9afd37a3d54615a049c69f1c80db1a?srsltid=AfmBOor6Mxq8BSucxHMlQrBFZfyGybsk3j_hLRcltRvAo2BVOLfisani]]\\



====Variations====
  * Use sodium hydroxide solution instead of copper(II) chloride to remove most of the aluminum, leaving behind only a fragile plastic "can shell."



====Safety Precautions====
  * Safety goggles must be worn.  
  * Copper(II) chloride is toxic if ingested and irritating to skin, eyes, and tissues. Avoid all contact.  
  * Check safety data sheet for sodium hydroxide before using.  
  * Torn aluminum cans have sharp edges; handle with caution.  
  * Clearly label solutions and do not leave them where they may be mistaken for drinks.




====Questions to Consider====
  * Why does copper(II) chloride react with aluminum but not the other way around?  
  * What role does the plastic lining inside the can normally serve?  
  * How does the activity series of metals explain the outcome of this demonstration?  
  * What would happen if a less reactive metal salt, such as zinc chloride, were used instead of copper(II) chloride?  
  * Why is warm water recommended for dissolving copper(II) chloride?