what is the redox reaction for art restoration? what is the importance and application of the reaction?
151970
1)The rxn for art restoration is oxidation, which is part of the redox rxn. \n2-3) Oxidation is used in the production of cleaning products; and these products can be used for art restoration.
129663
Please do your own home work.\n\nI suspect you are missing a symbol, it probably should be,\nN2O4  <==>  2NO2\n\nThink about how each of the changes will effect the equilibrium of the reaction.
988889
understanding the reaction meachanism \neffect of catalysts etc....\ndetermining the amounts needed
139943
corrosion is normally the oxidation of the metal, painting it stops the air getting to the metal and therefore stops the oxidation.
118571
corrosion is actually oxidation. A chemical reaction between oxygen and various materials such as metal. Painting metal prevents oxygen from reaching the metal and stops the chemical reaction.
834819
Without knowing what reaction you're trying to get, or everything else present, thats a difficult question to answer.\n\nIn a sense. you're forming a silver nitrate solution, but you have to knw all the spectator ions to know what reaction will actually occur.  The silver cation in solution needs to have a anion associated with it.  \n\nThe purpose may also have something to do with the variable solubilities of the silver compound that may be formed.  \n\nAnother potential reaction involves the nitrate as an oxidizing agent.
828740
fe is the reducing agent cos fe undergo oxidation prosess changing its oxidation no from 0 to 2+
971763
1) Fe(s) +Cu^2+(aq) --> Fe^2+(aq) + Cu(s)  Single replacement, redox reaction where iron is oxidized and copper is reduced\n\n2) 2Al(s)+(3/2)O2(g)-->Al2O3(s)\nredox reaction, oxygen is reduced (neutral to -2) and aluminum is oxidized (neutral to +3)
837948
Articles from the HTPAA Quarterly Publication - Tool Chest  \n\nFeatured Article on Rust Removal\nPart 1 - Electrolysis\nHome  \nElectrolytic Removal of Rust \n\nby Kevin Chamberlain, Member HTPAA ( published in Tool Chest #63, February 2002) \n\nIntroduction \n\nAt our last Tool Conference, there was a Panel Discussion dealing with the cleaning and restoration of old hand tools. This is a key concern for anyone interested in collecting old tools, since one rarely finds tools in mint condition in an original box. It is much more common to find tools showing the combined effects of correct usage, abuse, neglect and simple ageing. The primary question is: should cleaning and/or restoration be attempted at all?\n\nThe answers are conflicting; some aim to restore the tool to a brand-new appearance, eliminating all evidence of its life history. Others think any attempt at restoration will destroy the character and value of an antique tool. \n\nMost think some intervention is desirable to remedy the effects of abuse and neglect, while still retraining as much patina and character as possible. There is an important caveat - "when in doubt, do nothing". Cleaning and restoration of antique tools should be done in a careful and meditative mood - otherwise rash actions may cause loss of valuable information and/or further damage. \n\nRemoval of rust from old tools or other artefacts may or may not be a desirable goal. In some cases (museum specimens) stabilization to prevent further deterioration may be all that is necessary. Rust may be regarded as undesirable by tool users or collectors because it obscures identifying marks, causes seizure of moving parts, creates an unpleasant rough texture to the touch, stains the hands and/or the workpiece, or is simply unsightly. I believe rust removal is often justified, but the method chosen should not alter the surface in other ways and should result in a reasonably attractive surface appearance.\n\nThe electrolytic method of rust removal meets these aims very well and is also a gentle, cheap and adaptable method. Electrolysis is now being used by a wide range of artefact restorers, from tool collectors to marine archaeologists. \n\nIn this article, I mainly aim to outline the practical aspects of the electrolytic method so that members can try it for themselves. Several HTPAA members have been using the method for some years and find it very useful\n\nWhat is Rust? \nRust arises from the surface oxidation of iron or steel in the presence of atmospheric oxygen and moisture. As the rust forms, the surface of the iron is eaten away, sometimes evenly, but often deep local pitting occurs beneath wart-like protuberances. Rust occupies more volume than the iron it replaces, and so moving parts will tend to seize as they rust. \nChemically, most red rust is hydrous ferric oxide FeO(OH). If water enters this chemical structure, yellow-brown limonite may form FeO(OH).nH2O. Quite often, black iron oxides are also present usually magnetite (Fe3O4), an iron oxide which both conducts electricity and can be magnetised. The rusting process, and the conditions which promote, inhibit or stabilise it, are all important topics which are beyond the limits of the present article. \n\nMethods of Rust Removal\nRust usually binds strongly to the underlying iron or steel. Various methods have been used to remove rust. Mechanical methods include the use of emery paper, sandpaper or wire brushes (either manual or powered). More aggressive methods include sand blasting or shot blasting. Plastic bead blasting is a more recent and gentler variant. Clearly these methods will scratch the metal surface if the abrasives are harder than the metal. Wire brushes, for example, do not appear to scratch hard steel surfaces but they can be quite damaging to soft iron surfaces. \n\nGas flames are sometimes used to dislodge rust, relying on the different expansion rates of the oxides and the metal in response to heat. Simple bo
610699
Pb(NO3)2(aq) + H2SO4(aq/l)[depending on concentration] --> PbSO4(s) + 2HNO3(aq)\nPb2+(aq) + SO42-(aq) --> PbSO4(s)\n\nI don't see how an redox reaction could occur.
559378
Sulphuric acid is a strong oxidizing agent and does not complex ions easily. It thus is a wonderful reagent to activate ions for study.
170896
You dip the metal you want plated into a solution containing ions of the metal you want to plate with, such as chromium (chrome).  The dipped metal is attached to an electrical current, which induces a redox reaction.  The actual chemistry is a little more complicated, but the easy version is that those metal ions become solid metal attached to the electrode (the metal that you dipped in the solution).  The new metal is now permanently bonded to the old metal, and you have a set of chrome rims.
167656
the correct answer is B. A is wrong b/c it isn't an oxidation reduction reaction. Looking at a table of solubility products will confirm the answer is B.
200542
There is no active ingredient per se.  The better grades of paint use titanium dioxide to create the whiteness and to assist in covering.
302323
Although the type of corrosion most of us are familiar with involves molecular oxygen, corrosion, in general, does *NOT* require the presence of free oxygen.  \n\nFor example, galvanic corrosion, which can occur when two dissimilar metals with different oxidation potentials are in electrical contact.  The less noble metal will form an anode, and be oxidized, while the more noble metal will form a cathode, where reduction reactions will occur.  In the absence of oxygen, reduction reactions like:\n\n  2H+ * 2e- -> H2(gas)\n\ncan occur.  This reaction is particularly important in acidic environments, (when the H+ concentration is high).  Such environments can develop in corrosion environments via hydrolysis reactions, e.g., \n\n  Fe3+ + 3H2O -> Fe(OH)3(solid) + 3H+\n\nwhere the Fe3+ ions are produced by the oxidation of iron metal, and Fe(OH)3 is the solid mineral "goethite", a major component of "rust".\n\nCorrosion can also be induced in the absence of free oxygen by the action of some species of bacteria. For example, there are bacteria that can reduce sulfate ions (SO4--) or nitrate ions (NO3-) to hydrogen sulfide (or metal sulfides) and molecular nitrogen.  To do so, they need to couple these reactions to a "source" of electrons, which can be a metal surface that is then oxidized (i.e., corroded). \n\n\nFinally, there are some metals that are themselves strong reductants -- so strong that they can reduce water.  Li, Mg, Na, and Al all have standard oxidation potentials that are lower than that of water, so they will react spontaneously (in the case of Li and Na, *violently*) with pure water (even water containing no free oxygen) to form metal ions or hydroxides and hydrogen gas.
652769
Galvinisation with zinc. \n\nChroming\n\nboth work off the basis of reduction and their poteintal to be oxidised\n\nlook in an chemistry A-Level text book. Or if your american look at a college text book, for exact details
1029176
There is a school of thought that there is no such thing as sulphurous acid, that what is referred to as sulphurous acid is merely a solution of sulphur dioxide in water,\n\nHaving said that, "sulphurous acid" is a mild reductant and might reduce aqua regia, which is a strong oxidant due to the nitric acid content.  In practice, dilution would be more important than than the reduction using sulphurous acid but you could get the effect by bubbling gaseous sulphur dioxide through the aqua regia.\n\nIn point of fact, I have my doubts whether sulphur dioxide would act as a reductant under these conditions; I suspect the kinetics would be very slow.  If it did, you might see reduction of gold to metal or possibly precipitation of gold chloride.