Was anyone able to balance this??? I did the work, came up with CuO as the stuff, But can't seem go convince myself that the balance works, can someone please let me know what the balanced equation for this problem in the end is?? thanks
A hydrate is a chemical compound that has water molecules bound loosely to it by electrostatic forces. When the hydrated compound is heated, the water molecules are released as water vapor. The formula of the copper carbonate hydrate, Cu2CO3(OH)2*H2O, tells us that one water molecule is bound to each copper carbonate hydroxide molecule.
From the ratio of the mass of the black product to the initial 5 g placed in the flask, could the remaining black compound be the anhydrous copper carbonate hydroxide molecule Cu2CO3(OH)2? The molecular weight of Cu2CO3(OH)2 is 221.116 g/mol, while that of water is 18.015 g/mol. Be sure to show details of your calculations.
(After I heated, there was 3.327g of black powder, so 1.673g of H2O boiled out.) After some math I figured out that since the one to one ratio of Cu2CO3(OH)2 and H20 that there is 5.6 x 1022 of water molecules and since the 1 to 1 ratio, would equate to approx 20g of the Cu2CO3(OH)2. So this is how I deemed it was not the anhydrous copper carbonate hydroxide molecule Cu2CO3(OH)2.
2. If the product is NOT anhydrous copper carbonate hydroxide, perhaps the black color provides a hint as to its identity. Identify the product from the following list of copper compounds:
CuCO3 - light green powder
Cu(OH)2 - blue green powder
Cu2O - reddish brown crystals
CuO - black powder
Since all I was given was the above choices, I equated a black powder to CuO and left it at that.
3. Write a balanced equation for the observed decomposition of copper carbonate hydroxide hydrate