What does an active metal release from an acid?
481911
H2, or hydrogen gas.\n\nFor example, take magnesium metal and hydrochloric acid.\n\nMg + 2HCl -> H2 + MgCl2\n\nThis is a displacement reaction, in which a free element (Mg) breaks the bond between a compound (HCl) and then bonds to the ion with the opposite charge (Cl-) forming a new compound (MgCl2).  The ion left over (H+) loses its charge and becomes a pure element (H2).
492103
Assuming the spring doesn't release that bit of its potential energy as kinetic energy by decompressing as it falls, it will be released as kinetic energy as the pieces of the disintegrating spring are forced apart due to the stress placed on the object and the action of the acid weakening its structure (there's no such thing as instantaneous disintegration... even if it only takes a millionth of a second, it still took some time to happen).\n\nBeyond that, quite a bit more chemical energy will be released as the acid oxidizes the metal in the spring and causes it to disintegrate.
185295
sodium hydrogen carbonate: [Na+][HCO3-].\n\nThe anion can release a proton:\n[HCO3-] -> H+ + [CO3(2-)]\n\nTherefore it can behave like an acid when it encounters a base, e.g.:\n\n[HCO3-] + NaOH -> [Na+][CO3(2-)] + H2O
40274
The magnesium metal buried nearby provides protection from corrosion.  “Corrosion” is the technical name for the chemical reaction that takes place when a metal combines with oxygen.  Magnesium acts as an anode and protects the iron or steel tank by corroding in preference to the iron or steel tank.  This means that instead of Iron giving up electrons that attach to the oxygen atoms(which causes corrosion), the Magnesium releases the electrons.  The Magnesium and Oxygen atoms combine to form magnesium oxide while Iron does not take part in the chemical reaction and is thus protected.\n\nThe corrosion of a magnesium anode in preference to steel is an example of galvanic protection.
1054682
It "fizzes".  When you put acid on CaCO3 it reacts to release CO2 gas:\n\nCaCO3 + 2H+(aq)  -> Ca2+(aq) + H2O + CO2(g)
454802
it's basically from the movement of electron transfer from one of the metal to the other. to know the flow of electrons from which metal to which, u need to know their standard reduction potentials
1024027
Copper in the metal spark and flame apparatus of the lighter.  The metal is heated by the flame, and electrons in the metal are excited and jump up a few orbitals (energy levels), and on the way back down to the ground state, they release the energy in the form of light correpsonding to green wavelengths.
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.
933780
CO2 and H2SO4\n\n"metal" belongs to group IA, IIA, and B\n\nNa is IA\nK is IA
59524
...as an antacid\n\nneutralizes acid by releasing carbon dioxide.
625286
Cu is more active than Silver or to put it in more technical terms, its reduction potential is higher. Thus this particular reaction is spontaneous i.e. happens on its own. \n\nThe reverse is also possible but only if you supply the energy required which is usually in the form of electricity.
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)
885673
Not sure what you mean by "active", but  elements vary in how reactive they are (like how easily they bond with other elements) according to their position in the periodic table. \n\nLook up "Chemical Reactivity" in your text or on the internet. There's a fairly clear explanation here:\nhttp://www.sciencebyjones.com/chemical_reactivity.htm
372993
If you mean the decomposition of a chemical (electrolyte) by the passage of an electric current, you just get two electrodes (pieces of metal) that won't be attacked by the chemical or its electrolysis products and stick them in the electrolyte, and then connect the electrodes to a source of electrical current. You have to experiment with the voltage to be sure it is enough to produce electrolysis at a reasonable rate. If you want to collect any gaseous products of electrolysis, you can let the gas bubble up into an inverted container that is initally filled with the electrolyte. \nElectroplating (ref.) is a related phenomenon. In this case one electrode, connected to a negative voltage, is the metal item you want to receive the plating and the other, connected to a positive voltage, is the metal that provides the plating. The electrolyte is a water solution of a salt of the plating metal.
446541
An acid and a base react to form a salt and water.  For example:  NaOH + HCl ==> NaCl + H20.  The products will always include some sort of salt, as well as water, and the reation will always be exothermic, meaning energy is released.
1002183
Concentrated Nitric Acid and copper.  Be careful.  Nasty stuff... really!
445950
As the metal flexes, the molecules which make up the compound are temporarily displaced and generate kinetic energy which is dissipated as heat.   The process can be demonstrated in reverse i.e. when metal is heated, the molecules are displaced and the metal becomes pliable