A copper penny dropped into a solution of nitric acid produces a mixture of nitrogen oxides.....?
367815
Try finding the standard reduction potential for Cu and NO first then use those poteintial rxn equ to form the above full reaction afterwhich simply add or substract the poteinital u find to get E for the above reaction. \n\nSince E is proportional to the rate constate, u can use the above concentration as well as partial pressure to calculate the rate constant and hence E. Taking care that rate constant is the concentration/partial pressure of the reactant over the product!
707894
Cu 2+ ClO3 1-\n\nCu(ClO3)2
535149
Actually the copper doesn't come directly from the solution...\n\nNot sure how much detail you want, but it does use electroplating.  This means that it uses electricity to plate metal on an object.  The stainless steel object is put on the "positive end" and a lump of pure copper is placed on the "negative end."  A low voltage is used because a high voltage plates too fast, and the layer will peel off quickly.  If copper is the plating, then the solution must be a fairly low-concentration copper sulfate (CuSO4) solution, meaning that copper is the only metal present in the electrochemical cell.  The negative end is called the anode, and this decreases in mass as its copper ions are taken to the positive end -- the cathode.  \n\nThis method of plating multiple metals is actually fairly common, because the properties of each one can be combined.  Nickel can be used for farm equipment and engines because it can withstand a lot of force, silver is used for decoration, chromium is used to withstand a lot of use (like a spoon).  Copper is able to conduct heat and helps food cook evenly.
279857
I have no idea what you are asking, would you like to rephrase the question?\n\nNitrate is an ion....a poly atomic ion with chemical formula NO3 with a super script -1, indicating it has a negative 1 charge over the entire ion.  Nitrate is an anion, meaning it has a negative charge, it will combine with cations (+) to form ionic compounds.\nCations and anions combine so form an overall neutral compound.\n\nFor example, in the case that Nitrate combines with a Potassium Ion to make Potassium Nitrate, the formula is,\nK+ + NO3- --> KNO3\nSince Potassium has a +1 charge, only 1 Nitrate is needed to make an overall neutral compound, however, in the case of a Calcium ion combining with Nitrate,\nCa+2 + NO3- --? Ca(NO3)2\n2 Nitrates are needed to balance the +2 charge on Calcium.
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)
831216
Cu (s) + Pb(NO3)2 (aq) ---------> No Reaction. \nCopper will not replace lead.\n\nreaction VI in the attached link.
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
953754
Of course, it is a chemical reaction that causes ths to happen naturally.\n\nExpose the silver article to sulphur. SO2 would do the job most admiarably. Dipping it in egg yolk too - it is the sulphur that does the job.
1018313
Silver is being oxidized, nitrogen from the nitrate is being reduced.\n\nOxidation half reaction:\nAg --> Ag+  +  e\n\nReduction half reaction:\nNO3- +  4H+ + 3e  -->  NO + 2H2O\n\nNet balanced and reduced equation:\n3Ag +  NO3- +  4H+ --> 3Ag+ + NO + 2H2O
596804
3Cu+8HNO3=3Cu(NO3)2+2NO+4H2O
1908
Nitric acid is a highly oxidizing acid, and when combined with stainless steel will promote oxidation of the chromium content of the steel, creating a film that will protect the steel from further attack by the acid. Stainless steel is a recommended container for nitric acid. \n\nHydrochloric acid is less likely to undergo this interfering oxidation reduction reaction, leaving the steel unprotected, so even though it is a weaker acid, it will dissolve the steel. \n\nSometimes the turtle wins the race.
876773
The first reaction is simply wrong.  Nitrous acid does not ionize to nitrate.\n\nThe second reaction is a precipitation reaction, showing the net ionic equation.  The compound is ionic.\n\nThe third reaction is an example of SN2 displacement, not elimination.  Only single bonds are formed.
744530
It is an electrophilic aromatic substitution reaction.  Because the -COO- acts as an electron withdrawing group to one phenyl group and a moderate electron donating group to the other pheny group the nitration will occur on the pheny group where the COO- is acting as an electron donating group.  The major product of the nitration will have the -NO2 in the para position because the ortho position is partially blocked by the large COPh group.\n\nI hope this helps!
888667
Cu2S + 12HNO3 -> Cu(NO3)2 + CuSO4 + 10NO2 + 6H2O\n\nThere you go.
916549
2Cu + O2 ---> 2CuO,          \nThis is copper oxide or cupric oxide or copper( II )oxide\n\n4 Cu + )2---> 2Cu2O\nCopper also combines with oxygen as Cu2O, cuprous oxide , or copper(I) oxide
207493
Copper (II) nitrate, Cu(NO3)2, is dark blue.\nBarium nitrate, Ba(NO3)2, is white.\nIron (III) nitrate, Fe(NO3)3, is purple-greenish.\nLead (II) nitrate, Pb(NO3)2, is clear or white.\n\nNot sure what the orange is, but it's not one of those.
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.