would aluminum displace copper from a copper solution? and why?
Use the coffee tinsJust coat them with cooking spray and fill 1/2 full with your doughLet rise and then bake per your recipe instructionsThey will cook beautifully and be just the right size when sliced to make the perfect sandwichI always save my 'tins', especially at this time of year when I am doing a lot of Christmas baking.
You don't need any kind of pan to bake breadJust form it into a rough loaf shape, put it on a cookie sheet or baking sheet, and pop it into the ovenDont forget to score the top with a sharp knife several times to allow the innards to expand.
I don't think soThey probably weren't designed to withstand high heatAnd I would be particularly concerned about potential carcinogens from any paint or coatings on the tinsMaybe you could fashion something out of regular aluminum foil? Do you have anything made of oven safe glass? Caste iron? Dutch oven?
Do you have a cast iron skillet? Or pyrex? I have successfully made bread in both of those in addition to bread pansIn regards to cans, I have baked in cans but they have been thicker metal cans like coffee cansI don't believe aluminum would be a problem as long as they were food and heat safe to startFor example you could probably cook in green bean cans but not a coke canJust an educated guess.
Sort ofBased on the fact that aluminum is above copper in the activity series, we would predict that aluminum metal will be oxidized as copper(II) ions are reducedThe catch is that it often doesn't work out the wayFrequently, all one ends up with is wet aluminum, but no reactionAluminum is covered with a passivating layer of aluminum oxide, Al2O3, which prevents the aluminum metal from reacting with the copper ionsAcids will react with the Al2O3 layer, as will hydroxide ions and even chloride ionsAl2O3(s) + 6H+ - 2Al^3+ + 3H2O(l) Al2O3(s) + 2OH- + 3H2O(l) - 2Al(OH)4^- Al2O3(s) + 8Cl- + 3H2O(l) - 2AlCl4^- + 6OH- A common demonstration is to add aluminum foil to a solution of copper(II) ions and observe that no reaction occursBut when NaCl is added to the solution, a reaction occursIf aluminum metal is added to a solution of copper(II) chloride then all the ingredients are present to allow a reaction to occurChloride ions react with the oxide coating and aluminum metal reacts with copper(II) ions2Al(s) + 3Cu2+ - 2Al3+ + 3Cu(s)
