what would be the reaction to take place of aqueous copper (II) sulphate solution with graphite electrodes?
483935
I'm not sure what you mean by reaction to take place *of* copper sulphate...  There is a reaction that takes place *at* the electrodes.  If you use a set of graphite electrodes, the anode is unaffected by the electrolysis.  The cathode will slowly develop a film of copper, first on the bottom of the electrode and then moving upward.  \n\nThere is no actual reaction between the electrodes and copper sulphate, because graphite (and platinum) electrodes are inert.
639328
(NH4)2S.  Cu2S is dark in color.
801118
CuCl2 + 2NH4OH --> Cu(OH)2 + 2NH4Cl\n\nCu(OH)2 (s) + 4NH3 (aq)     ----->     Cu(NH3)4^2+
339643
You need a reference table and some instruction. Go to this site and scroll down to electrochemistry. Good luck!\nhttp://spiderpong.sitesled.com/chemistry_12_handouts.htm
750179
NaCl2 + NaCO3 ==> NaCO3 + NaCl2 NOTE: these two reactants will not react because the reactants and the products are identical\n\nCu + O2 ==> CuO2   This is already balenced\nCuSO3 + Fe ==> FeSO3 + Cu   The charge is not given so procuts could be different\n\n2HCl + 2Zn ==> 2ZnCl + H2\nMnO2 + H2O2 ==> No reaction: similar to NaCl2+NaCo3\n\nGood luck
581638
Galvanic corrosion tends to occur when dissimilar conducting materials are connected electrically and exposed to an electrolyte. The following fundamental requirements therefore have to be met for galvanic corrosion:\n\n   1. Dissimilar metals (or other conductors, such a graphite).\n   2. Electrical contact between the dissimilar conducting materials\n      (can be direct contact or a secondary connection such as a common grounding path).\n   3. Electrolyte (the corrosive medium) in contact with the dissimilar conducting materials.\n\nWhen placed in an electrolyte, different metals/alloys assume different corrosion potentials (refer to the galvanic series in seawater). It is this potential difference that is the driving force for galvanic current flow. The less noble material in the galvanic couple will become the anode and tend to undergo accelerated corrosion, while the more noble material (acting as a cathode) will tend to experience reduced corrosion effects. However, in some cases, chemical species produced at the cathode can degrade certain cathode materials.\n\nIt is not only the potential difference that controls the magnitude of galvanic current flow. The total resistance to current flow (see schematic of a simple corrosion cell, with both arrows showing conventional current direction) also needs to be considered, which can be broken down further into the following individual resistance components:\n\n   1. Resistance to (ionic) current flow of the electrolyte.\n   2. Resistance to current flow (by electron conduction) in the conducting materials and in the connection between them.\n   3. Resistance associated with polarization behavior of the anode.\n   4. Resistance associated with polarization behavior of the cathode (cathode efficiency).
788768
Just the usual stuff.  Use an electrolyte (H2SO4/HNO3), a couple of electrodes, a reduction table of half cell potentials, and some electricity.
308525
Yes.  If carried to the extreme, you would see the aluminum strip dissolve, copper metal precipitating, and the solution color will fade from blue to colorless.\n\n2Al + 3Cu(2+) ---> 2Al(3+) + 3 Cu
1087032
try Vogel's "Qualitative Inorganic Analysis", I'm pretty sure it has all the answers 4 u.\n\ndont care editions, but for 7th ed, ISBN is 0582218667\n\n****\nokey then, from Vogels\n\n1) when heated, lead nitrate decomposes to white solid lead oxide (PbO), brown gas (NO2) and oxygen gas. Brown gas decolorizes when contact with water. \n\n2) ammonia odur. ammonium compounds are all volatile towards heat and decomposes to ammonia and an acid but quickly recombine if the acid, in this case, hydrochloric acid, is a strong acid.\n\n3) anhydrate copper sulphate is white, hydrate copper sulphate is blue. I have no idea which one you actually heated. If it's anhydrate, no change; if hydrate, blue ---> white.\n\n4) blue precipitate forms initally, but resolve upon excess reagent, clear blue soln results due to the formation of copper complex [blue precipitate: Cu(OH)2*CuSO4, complex: [Cu(NH3)4]^2+]\n\n5) brown precipitates froms [Cu(OH)2], no change with excess reagents.\n\n6) metal-gray stipe (magnesium stipe) gains a redish brown color due to formation of copper metal. Possible decolorization of the soln (depends on how much magnesium u actually put in)\n\n7) volatile reaction, solid metal solves,ignitable gas is formed. (if phenolphthalein is added to water initally, soln becomes pink)
195781
None. "A more active metal will displace a less active metal from a solution of its salt." Copper and lead are both less active than zinc. Obviously, zinc won't displace itself from zinc sulfate.
500112
Even though it may seem like copper won't react with nitric acid because copper is lower than hydrogen on the reactivity series, whoever believes so would be mistaken.  Although it's true that a double-replacement (metathesis) reaction would not occur, an oxidation-reduction (redox) reaction does occur:\n\nCu + H+ + NO3- ---> Cu2+ + NO + H20 (unbalanced) \n(Note: the colorless NO gas immediately reacts with the O2 in the air to form brown NO2 gas)\n\nThere isn't really such a thing as the neutralization of copper, you can chemically change copper metal to copper ions, which are soluble.  Through this reaction, you can "dissolve" copper metal.  Dissolving, though, isn't exactly the right word because dissolving is a physical procedure, but this procedure is a chemical one.
529595
The is no specific wet test that would involve reagents that you would be able to get.  They are pretty exotic reagents.  Much cheaper would be to take a sample to a local lab and pay $25 or so for a copper test.\n\nIf there are no other metals believed present, you can do this.  Take the solution or solids and acidify until dissolved. Filter any solids left and decant.  Add ammonium hydroxide (15M) to the decant until the solution is slightly basic.  If the solution is not blue, copper is not present in more than trace levels.  If it is blue, add acetic acid (5M) dropwise until the blue color just disappears.  Then add 2 drops of 0.2M K4Fe(CN)6.  The formation of a red solid confirms the presence of copper.  Note this only works if copper is the only metal above impurity levels.\n\nTo see if chloride is present gets very complicated by wet methods.
418443
Copper can react with nitric acid on two different ways based on the concentration of nitric acid.\n\nIf cold and dilute nitric acid is used, then the reaction yields copper(II) nitrate, nitrous oxide(N2O) and water.\n\nCu + HNO3 ----- Cu(NO3)2 + N2O + H2O\n\nIf hot and conc. nitric acid(a stronger oxidising agent) is used, the reaction yields copper(II) nitrate, nitrogen dioxide(NO2) and water.\n\nCu + HNO3 ----- Cu(NO3)2 + NO2 + H2O\n\nP.S. - Balance the equations yourself(might take some time but use the oxidation no. method)
1049419
This is a very old lab experiment.  You make a strong solution of copper sulfate in water, put the solution in dialysis tubing suspended in a container of plain water, and watch the diffusion occur.  Eventually, the solution will be balanced inside and outside the tubing.  I think they use copper sulfate because of the vivid blue color.
469693
Nothing. The two reactants have the same anion, so no reaction will take place. If you create a hypothetical double displacement reaction, you get:\n\nFeS + CS2 --> FeS + CS2\n\nAnd, so, there is no reaction.
203972
I've done some research on this because I seem to remember my teacher talking in school about how they can make batteries with graphite (pencil lead) and vinegar that put out more energy and are more environmentally safe than regular batteries. I'm not sure how this happens but I know that you can take vinegar and pour some into powdered graphite, rub it into a block of wood, and when the vinegar dries the wood will be extra strong because the vinegar disolves the graphite long enough for it to bind to the wood. I can't find any research or projects to back this up but that is what I remember on the subject. Perhaps you could split a pencil and drop the lead in for a few days and see? Maybe use two and a nine volt battery and see what a current does to affect the chemical process...I wish I could help you more.
857898
2Al + 3*(CuO) -> Al2O3 + 3*Cu\n\nI2 + 2*(Na2S2O3) -> 2*(NaI) + Na2S4O6\n\nI2 + 5*(Cl2) -> 2*(ICl5)