This lab was about aluminum reacting with copper (II) chloride. On day one of the lab, we allowed aluminum to react with copper (II) chloride in a beaker filled with water. On day two, we removed the chunks of wet copper (the product) from the beaker and put them on a sheet of filter paper. Finally, on day three, we measured the mass of the dry copper. It was determined that aluminum was the excess reagent and copper (II) chloride was the limiting reagent. There are a few post lab questions that I need help with. Here is a chemical equation to help you: 2Al+3CuCl2 -gt; 2AlCl3+3Cu Which gas was produced in this lab (in Day 1)? State evidence of a gas being produced? Why did the blue color of the solution disappear? (Day 2) Describe the appearance of the product. (Day 2 before filtering) Why did the product have that particular appearance? Thanks for the help!
Get a Quiet one. I am tired of all these FARTING exhaust.
Hi Evy, 2 Al(s) + 3 Cu(2+) + 6 Cl(-) 3 Cu(s) + 2 Al(3+) + 6 Cl(-) these are the ions Cu(2 +) that give the blue color to the solution . . . ! All Cu(2 +) ions reacted because Al is in excess . . . that is why the blue color disappears . . .
