How do Zinc batteries work?
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Zinc-carbon batteries, also called "Leclanché" batteries or dry cells, were invented in 1866. \nA zinc can serves as a container for the battery and as electrode (anode). \nA carbon (graphite) rod is placed at the center and used as the other electrode (cathode).\nThe space between the carbon rod and the zinc container is filled with a moist mixture of ammonium chloride, manganese dioxide, zinc chloride and carbon powder. \nThe chemical reactions produce electrons on the zinc electrode.  \nThe battery has a voltage of about 1.5 V, which decreases in time. The dry cell cannot be recharged or made to work again because the chemical reactions cannot be reversed.\n\nfor chemical reactions and more details see:\nhttp://en.wikipedia.org/wiki/Zinc-carbon_battery
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Generally chargable batteries are made from Ni-Cd or Ni-Mh and unchargables are Zn-C. If you wanna charge a battery, the electrons has to move in it. So,if you don't provide this you can not charge a battery...
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1) Litmus is red in acid, blue in base...so it would turn red in rainwater (which is sl acidic, more or less depending upon atm contamination), blue in ammonia.\n2) AgCl precipitates out...KCl + AgNO3--->AgCl(ppt) + K+ + NO3-\n3) Zn is more active than Fe, so it plates out at the expense of Fe...Zn(+2) + Fe--->Zn(ppt) + Fe(+2)\n4) Depends on the type of battery...for the lead/acid type it is a reversible reaction between PbO in the plates and the H2SO4 electrolyte (in overly simple terms)\n.....Discharge: 2H(+) + SO4(-2) + PbO--->PbSO4 + H2O\n.....Charge: PbSO4 + H2O--->PbO + 2H(+) + SO4(-2)
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there is a software called "accumulator training utility". this utility calibrate the "smart chipset" of a notebook battery.\nit does not work for defective batteries, for older and apple notebooks.\n\nhave a look for this utility on ebay in the category notebook batteries.\n\nin my humble opinion this utility is crap, but could work for batteries that have been always decharged only to 50% before recharging again.
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reduction:  2e- + Cu2+ --> Cu      Eo = +0.34 V  cathode (+)\n\noxidation:   Zn   --> Zn2+ + 2e-   Eo = +0.76 V    anode (-)\n________________________________________\n\nZn  + Cu2+ --> Cu  +  Zn2+         Eo = +1.10V therefore cell spontaneous as written.
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2 electrodes and a battery
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Electro-magnets use electricity to temporarily align all of the atoms in a ferrous material to a N-S position. When the electricity is turned off, the atoms return to their original misaligned state, losing much of its magnetivity. It never completely loses all of it, as some atoms will remain in the alligned state, creating a "Gauss" feild around it.
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Zinc has an atomic number of 30, so its default number of electrons is 30.\n\nHowever, 30 electrons isn't the most stable thing! The oxidation state of zinc is 2+, which means that it likes to have two less electrons than it's supposed to.\n\nIn summary:\nZn on its own has 30 electrons\nZn in an ionic bond has 30-2 = 28 electrons
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"Their intention is to try to make them last longer prior to use. I think everybody has had the experience of putting a bunch of batteries in a flashlight and then putting it in the trunk of their car, and they go back when they need the flashlight and it doesn’t work. Because just on standing, batteries actually deplete themselves. So the idea is that there’s a certain amount of chemical inside—it’s a chemical reaction that’s taking place in the battery—and the chemicals basically get used up. They basically just run out of active material.\n\nMost chemical reactions are affected by temperature, and the lower the temperature the slower the chemical reaction. So what people are trying to do is slow down the self-depletion mechanisms of the batteries by keeping them cold.\n\nIn general, it does extend the battery’s life. Whether there’s a significant difference that would be measurable to the consumer between room temperature and a refrigerator.... To be honest, I don’t know. But in general it does work—that if batteries are kept cooler while they’re not in use it will extend their shelf life.\n\nSo then what about the freezer? Is it even better?\n\nI think one would have to be careful about that. Because it’s the freezer, and the freezer is quite cold. Depending upon the type of batteries, you can actually freeze some of the internal components, and that would not be good. So probably the refrigerator is a safe bet and it will improve things a little bit.\n\nWhat if there are batteries that you’ve been using but will not use again for a while. Would placing them in the fridge in the meantime help at all?\n\nYeah, if you plan on storing them for a long time, it probably would. I think typically people put them in the refrigerator before use. Certainly people should not try to use the battery or activate the battery while it’s cold. It may not work very well. But if they let it warm up before they use it, it should help. \n\nWhat about batteries that are starting to run low?\n\n\nNo, that won’t help. When they start to run low they’re basically used up."
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You can figure it out.\n\nIf a neutral atom of zinc has an atomic number of 30, and a mass number of 65, then it has 30 protons, 35 neutrons, and 30 electrons.\n\nProtons and neutrons are found in the nucleus.\nSo, draw a circle. Write "30p+" and "35 n" inside it.\nThis represents the nucleus.\n\nIn Bohr's model, electrons orbit the nucleus at specific energy levels. The first level holds up to 2 electrons.\nThe second holds up to 8.\nThe third holds up to 8.\nThe fourth holds up to 18.\nWe use dots to represent electrons.\n\nDraw a ring around the nucleus.\nAdd two dots to the ring, usually at noon and 6:00.\n\nDraw another ring around the first one.  Draw eight dots: two at noon, two at 3:00, two at 6:00, and two at 9:00.\n\nContinue adding rings and electrons.\nYou should end up with twelve dots in the outermost ring.\n\n(Which doesn't correspond with the  Lewis diagram for zinc, but that's  another story....)
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Search the web for zinc and read the fact sheet - it offers a lot of information.  Good luck - hope you find the answers you're looking for.
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zThe zincs you use on a boat are called "Sacrificial Anodes". Zinc is used because it has a higher voltage in the water so the current will be more inclined to flow from it than from your propeller. To complete the electrical circuit, the zincs must be connected to the items they are intended to protect. Usually this is no problem because the zinc is bolted right to the shaft or underwater housing. Non metal boats will usually have a copper bonding wire inside that connects all the underwater metal items together so they all share the protection from zinc anodes. Since engines use the metal frame as the negative battery connection and the engine is connected to the prop shaft, the engine and the negative side of your 12 volt system are also part of this bonding connection. This bonding wire is usually connected somewhere to the rigging. This is not for electrolysis protection but for some protection from lightning strikes to conduct it into the water through the items connected together.\n\nBasically you put it there to stop your propeller and stuff from corroding...
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Heat speeds up the chemical reaction within the battery. This delivers lots of electrons from the positive terminal to the negative terminal. To the extent that these electrons are lost to the environment (i.e., if there are any conductors that can carry the electrons away from the negative terminal), the battery is being discharged, and a portion of its chemical energy has been wasted.\n\nThat's why many people store batteries in the refrigerator or freezer. Being cold slows down the chemical reaction, so there is less tendency for the battery to discharge. The battery won't provide much electrical power if you try to USE it while it is cold, but cold is a good way to store it and preserve its chemical energy for a future time when you warm it up and use it.
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Alkaline batteries contain basically Manganese Oxide and Dioxide coupled with Zinc oxide.  Manganese and zinc are known as transitional metals not alkali metals or alkaline earth metals.  The reason why alkalines batteries are called alkaline batteries is due to the potassium hydroxide electrolyte.  \nMixing an alkali or alkaline earth metal with a halogen will produce a salt known as a ionic salt.
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It certainly should.  Zinc is much higher in the "electromotive series" than is silver.  This means it would displace silver.\n\nZn (s) + 2 AgNO3 (aq)---> Zn(NO3)2 (aq) + 2 Ag (s)\n\nSolid zinc dropped into silver nitrate solution will precipitate silver.
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zinc metal cells form a mettalic lattice wherein the atoms form mettalic bonds - which are not as strong as chemical bonds - from oxidation
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Individual atoms in the battery are made up of a nucleus (protons and neutrons) surrounded by electrons.  The chemical reactions in batteries cause these atoms to gain or lose electrons so that electrons become free to be conducted to another atom, or conversely the atom that has lost an electron becomes open to accepting an electron because it has a hole where an electron used to be. This flow of electrons (or holes) are what is called electrical current. The potential between atoms is measured in volts. The flow of electrons is measured in amperes (or amps).