thermal decomposition of copper carbonate?
913627
Hey, i'm doing that for Chem coursework too! AS right?\nanyway, im not entirely sure, but the most important bit you need is a gas syringe to measure the volume of gas.\nOther bits u will need r:\n-conical flask on tripod, with bunsen underneath.\n-A bung with a glass tube in, to put in the conical flask.\n-This tube leads to the gas syringe, via a rubber seal.\n-Remember the CaCO3 goes in the conical flask.\n-Now all you need to do is heat the CaCO3.\n\nYour welcome!
978387
You should have gotten elemental copper via the following equation:\n\n3CuCl2 + 2Al ---> 3Cu + 2AlCl3\n\nThe water is not part of the reaction.
945429
Equation becomes CuCl2 + 2KI --> CuI2 + 2KCI\n\nProducts are Cuprous Iodide and Potassium Chloride
283215
[Cu(NH3)4]SO4*H2O (s) + 2HCl(aq) --->\n\nCu(NH3)4 +2 (aq) + H2SO4(aq) + H2O(l) + 2Cl-(aq)
95302
Cupric sulfate's heat capacity is described here.
808639
The answer given earlier is more feasible i.e decomposing sodium hydrogen carbonate, the equation thus:\n\n2NaHCO3 --> Na2CO3 + CO2 + H2O\n\nBut, the decomposition for your specific enquiry thus:\nNa2CO3 --> CO2+Na2O\n\nI hope this helps
825689
CuCO3 + H2SO4 --> CuSO4 + CO2 + H2O\n\nCu(OH)2 + H2SO4 --> CuSO4 + 2H2O\n\nFor the electrolysis:\n\nCuSO4 = Cu+2 (aq) + (SO4)-2 (aq)\n\nCu+2 (aq) + 2 e-1 --> Cu (metal)
413983
Copper sulphate as I recall.
793636
shawty's NOT good at stoichiometry...has made a fundamental error in the final line so end result is rubbish...\nhow can you end up with MORE Cu than you started with when it's 2 moles : 2moles? \n\n(8/159)x 127 = 6.4 g
211591
Ca3PO4 and CuOH\n\n^^those are the answers
394775
2Cu(NO3)2 ----> 2CuO + 4NO2 + O2\nOBSERVATION: brown, choking fumes of NO2 evolved; black solid i.e CuO settles at the bottom\n\n2FeSO4 ----> Fe2O3 + SO2 + SO3 \nOBSERVATION: white fumes of SO3 evolved and reddish brown solid i.e. Fe2O3 formed\n\nEDIT: The above equation for iron(II)sulphate may be a supposed characteristic for its thermal decomposition relating to that of copper(II)nitrate above, but Chaos, O2 will not be evolved here, because SO3 will not get reduced to O2, even on strong heating.
810145
depends what the magnesium is for. If this is for a chemical reaction, it's because copper is less reactive than magnesium (it's lower on the activity series list).
611161
Silver carbonate, Ag2CO3.
1025045
CuCl in Fire works\n\ncopper compounds + chlorine producer \ncopper acetoarsenite (Paris Green), Cu3As2O3Cu(C2H3O2)2 = blue \ncopper (I) chloride, CuCl = turquoise blue
205870
CaCO3(s) + 2HC2H3O2(aq)-> Ca(C2H3O2)2(aq) + H2O(l) + CO2(g)
787309
There is some research in this area.  There apparently are two types of decomposition.  Most references I see list 400-500C, but the research reference gives two temp ranges.
903862
Sorry Voyager. Copper is not so reactive a metal that it will react with sulphuric acid.\nYou need either solid copper (II) carbonate or solid copper (II) oxide for the salt.\nSince it is a sulphate, sulphuric acid is used together with the solid.\nHeat the acid so that the reaction can proceed at a faster rate. Add solid till no more will react (no bubbles of gas produced, and the solid remains insoluble). This is to ensure that all the acid is used up. Filter to remove unreacted solid and heat the filtrate, which is the copper (II) sulphate solution, till saturated (approximately 1/3 to half the original volume left would be a good gauge). Let the hot saturated copper (II) sulphate solution cool and after some days, when the excess water evaporates off, you should get hydrated copper (II) sulphate crystals.\nDo not heat till dryness as this will evaporate off the water of crystallization needed for the blue copper (II) sulphate crystals to form. Without the water of crystallization, you would get anhydrous copper (II) sulphate powder (white) and not the blue crystals.\n\nHope this helps :)