There is no gas as a product of the reaction. The bubbles you see there are just boiling water (solution) due to the highly exotermic reaction. This is a simple redox reacton:
Cu2+ (imagine as superscript) + Al – –> Cu + Al3+
im afraid to say that is wrong :/ Cu+ is colourless due to its complete d-subshell. it is greeny blue due to the copper(II) chloride impurites. and in fact they are both not even green or blue unless hydrated (by either moisture in the air or in solution)
17 likes for something totally wrong lol. Copper(I) itself is d-10 and colorless, it is usually insoluble and unstable in aqueous solutions. Copper(II) sulphate is blue because [Cu(H2O)6]2+ is blue; For copper chloride copper makes a yellow complex ion [CuCl4]2- therefore copper(II) chloride appears more green than blue.
As far as the gas goes it's probably a mix of steam (from the heat) and HCl; aluminium chloride, once formed in aqueous solutions, will hydrolyze immediately to form Al(OH)3 and HCl. I suspect that the reaction won't be as spectacular if one uses copper sulphate instead of copper chloride because aluminium sulphate doesn't hydrolyze as much as AlCl3 (but I could be wrong)
I did this experiment as part of a larger one in my Chem class. We started off with some copper wire and went through a few different compounds of copper and ended up with this. Really fun except we just put some aluminium foil into our beaker and saw it go from there and decanted the solution from there.
No, no no. The truth is much more complex than that. Notice how the crystals are all green, and a concentrated solution is green? Contrary to what simply high school chemistry teaches you, copper almost never exists in solution as the unbound ion, it bonds with suitable ligands to form a complex. The green crystals probably results from the excess HCl contamination in the crystals, forming a negatively-charged complex CuCl4(2-) via the attraction of the positively charged-cont
Cu2+ ions to the Cl- ions and acts as the ligand instead of water, because not much water is present. When the copper (II) chloride dries, water still remains as the hydrate, CuCl2.2H2O, in which the crystal is still green because the Cu2+ is still bound to the Cl-, making this more like CuCl4(2-).2H3O+ (approximation). When you dilute this with more water, the copper instead becomes attracted to the water molecule, because there are more water molecules than Cl-, so-cont
The copper forms the typical complex erroneously called the Cu2+ ion, the [Cu(H2O)6]2+ complex/ion, which has a blue colour, instead of the green of CuCl4(2-). Please forgive me if I have made a mistake in my explanation, this colour difference is very complex indeed.
Yet, the label clearly states that it is a copper (II) chloride. Actually, the ligands in solution may alter its color quite substantially. Here, chloride ions make complexes with Cu2+ ion that appear green, but on addition of concentrated HCl it can even change color to yellow due to formation of [CuCl4]2- complex anion. On the contrary, copper (I) compounds are mostly quite insoluble in plain water and appear green because of copper (II) impurities.
this is a great video showing the reaction of metals in the reactivity series, aluminum is more reactive, so it takes the place of the copper and leave behind metallic copper. same thing happens when you introduce copper into a silver salt solution or even chloroauric acid as a result of dissolving gold into aqua regia. the less reactive metals like silver, gold and platinum will precipitate out of solution if you introduce copper or any or the more reactive metals.
@periodicvideos Is the first reaction 12CuCl2 + 2Al2O3 -> 12Cu + 4Al2Cl3 + 3O2 as the aluminium oxide layer is consumed, and then as the copper(II) chloride reacts with the aluminium metal, 3CuCl2 + Al -> 3Cu + AlCl3, forming the copper metal deposit ? Or is there some copper oxide formed?
Aluminum is a correct spelling, & the American (& Canadian) way of pronouncing it is also correct. British chemist & inventor Humphry Davy settled on aluminum by the time he published his 1812 book Chemical Philosophy. I think calling it aluminum honours Humphry Davy, who identified the existence of the metal base of alum.
I need to make a marble fall through an aluminum bridge with some sort of reaction. it needs to fall in 2-4 minutes. the Copper(ii)Chloride reacts too quickly. Should I decrease the molarity and use more?
I would like to modify aluminium cylinder head intake tracks with this process-could you direct me to a copper chloride supplier? It sure is nice to hear aluminium called by it's real name, you hear that much in the racing industries…