how is electrolysis done?
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.
29248
here's what you need:\n\n1.18-gauge copper wire (smaller gauge will work too,2. but 18-gauge is stiffer)\n3.Wire clippers\n4.Steel paper clip (Some people find that a 2-inch 5.strip of zinc works better) \n6.Sheet of coarse sandpaper\n7.Lemon\n8.Help from an older friend or an adult\n\n\nhere's what you need to do:\n\n\nHave your older friend or an adult strip 2 inches of insulation off the copper wire. Clip the 2 inches of bare wire with the clippers.\n\nStraighten out the paper clip and cut about 2 inches of the straightened steel wire, or use a 2-inch piece or strip of zinc.\n\nUse sandpaper to smooth any rough spots on the ends of the wire and paper clip or piece of zinc.\n\nSqueeze the lemon gently with your hands. But don't rupture the lemon's skin. Rolling it on a table with a little pressure works great. \n \nPush the pieces of the paper clip and the wire into the lemon so they are as close together as you can get them without touching.\n\nMoisten your tongue with saliva. Touch the tip of your wet tongue to the free ends of the two wires.\n\nYou should be able to feel a slight tingle on the tip of your tongue and taste something metallic.\n\n\n\nwhat you will discover\n\nThe lemon battery is called a voltaic battery, which changes chemical energy into electrical energy.\n\nThe battery is made up of two different metals (the steel paper clip and the copper wire). These are called electrodes, which are the parts of a battery where electric current enters or leaves the battery. The electrodes are placed in a liquid containing an electrolyte, which is a solution that can conduct electricity.\n\nIn a solution of water and an electrolyte, like the acid in the lemon, an excess of electrons collects on one end of the electrodes. At the same time, electrons are lost from the other electrode.\n\nTouching the electrodes to your tongue closes the circuit and allows an small electric current to flow. A single lemon produces about 7/10 of a volt of electricity. If you connected two lemons together, you can power an inexpensive digital watch (uses about 1.5 volts). (Use a length of thin, flexible wire to connect the silver wire of one lemon to the copper wire of the other lemon. Then attach thin wires from the other two wires in the lemons to where a battery's positive and negative poles connect to power the watch.)\n\nThe tingle felt in your tongue and the metallic taste is due to the movement of electrons through the saliva on your tongue.\n\n\n--well, i just searched for it. hope i helped in a way ^_^\n\n-paul
575608
Melt the whole mixture and do an electrolysis. Would be quite expensive a process, but might be the only possibility e. g. on the moon in order to produce oxigen. Melting heat might come from sun and electricity from solar panels.\n\nI understood in principle such a reaction is done to make aluminium from bauxite. But in this case the producers immediately use up the oxigen through burning carbon electrodes in order to win the melting heat.
167961
To put it simply,\nHydrogen fusion works by fusing two Hydrogen atoms into a Helium atom.  This process gives off a lot of energy, which is the source of the sun power.\nIt takes incredible heat and pressure for this nuclear reaction to occur, this is definatly not something you do in your back yard.\n\nFor more detailed info,\nhttp://en.wikipedia.org/wiki/Nuclear_fusion\n\nIt is quite easy to seperate Hydrogen gas from water in a process called "electrolysis".  By passing an electric current through water with a dissolved electrolyte, it is possible to split water into Hydrogen and Oxygen gas.  There are actually numerous other ways of producing Hydrogen gas, but non as well known as electrolysis.
95444
Some tips...\n--Use a strong electrolyte (substances that will break up into ions [almost] completely in solution), the higher the concentration, the better.  Also you need to be careful on which electrolyte you choose.\n--Try not to use an over volttage (a voltage over the minimum necesary to electrolisize the water.  Insread, try to use a very high current, higher current = more production of gasses.  To increase current without increasing voltage, reduce resistance.\n--Place the electrodes close together to reduce internal resistance in the cell.\n\nEven by doing these things, you cannot hope to get much better than about 50% efficency doing water electrolysis, maybe 65% if you are good.\n\nThere are yahoo groups out there devoted to just such a tast as Hydrogen production through water electrolysis (I have one infact), they can also give advice based on experience.
435767
most common way is not through elecrolysis, but extraction from fossil fuels:  Here is a list of the ways...notice in every case a large amount of energy is input-and in most cases this energy comes from coal burning  for electricity or oil...\nHydrogen can be produced using a variety of domestic energy resources - fossil fuels, such as coal and natural gas, with carbon capture and sequestration; renewables, such as biomass, and renewable energy technologies, including solar, wind, geothermal, and hydropower; and nuclear power. Specific technologies and processes are described below.\n\nThermochemical Processes\nSteam methane reforming: In this process, high-temperature steam is used to extract hydrogen from a methane source such as natural gas. This is the most common method of producing hydrogen; about 95 percent of the hydrogen we use today in the United States is produced using this process. \nPartial oxidation: Scientists are exploring a process that produces hydrogen by simultaneously separating oxygen from air and partially oxidizing methane. \nOther thermal processes: Other processes include (1) splitting water using heat from a solar concentrator, and (2) gasifying or burning biomass (i.e., biological material, such as plants or agricultural waste) to generate a bio-oil or gas, which is then reformed to produce hydrogen. \nElectrolytic Processes\nElectrolysis: In electrolysis, electricity is used to separate water (H2O) into hydrogen and oxygen. Current electrolysis systems are very energy intensive. The challenge is to develop low cost and more energy efficient electrolysis technologies. \nPhotolytic Processes\nPhotolytic methods: In photolysis, sunlight is used to split water. Two photolytic processes are being explored: (1) photobiological methods, in which microbes, when exposed to sunlight, split water to produce hydrogen, and (2) photoelectrolysis, in which semi-conductors, when exposed to sunlight and submersed in water, generate enough electricity to produce hydrogen by splitting the water.
843269
Use the Nickel Metal..Put your steel into a electrolysis solution of Nickle  electrolytes and charge it with electric anode and cathodes.
536437
In order to overcome the strength of the  oxygen-hydrogen bond of water, a force must be used to electrochemically decompose a sample of water.  This is called a decomposition voltage and it is roughly about 1.2 volts at 25 degrees C.  In the lab a little more voltage is necessary to have the reaction occur at an acceptable rate.\nThis requires a cathode and an anode to produce hydrogen and oxygen gas, and of course a voltage.  \nElectrolysis of water:\n4H+ (aq) +4e- ------ 2H2(g) reduction at cathode\n2H2(l) ------- O2(g) + 4H+(aq) + 4e- oxidation at anode\n\n2H2O(l) ------- 2H2(g) + O2(g) net reaction\n\nEnergy: DeltaGrxn = +474.4 KJ\n\nGood night and Good Luck.
788768
Just the usual stuff.  Use an electrolyte (H2SO4/HNO3), a couple of electrodes, a reduction table of half cell potentials, and some electricity.
430141
I will make NaOH from the electrolysis of brine(saturated NaCl solution) using graphite anode and mercury cathode. On electrolysis, sodium will combine with mercury to form sodium amalgam(Na/Hg). Then make that sodium amalgam to combine with water(H20) so that we can get NaOH.
234381
In order to do this you will most likley have to also apply a voltage to the wire in order to drive the reaction.  Also, the bridge between the 2 beakers must be conductive, so there has to be some sort of electrolyte soaked into the bridge.  i would suggest using a simple copper sulfide solution in the plating side of the cell, and using an iron electrode in the other beaker.  electroplating is sometimes quite complex so you may want to consult a chemist regarding your final setup.
162163
WOW, you are really doing an over kill if you just want to electrolisize water.\n\nPure water does not conduct electricity.  Water will only conduct when it has ions dissolved in it, the more ions, the better it will conduct.  Tap water does have a small concentration of ions in it,  not much, but enough to make it conduct when you pass 30 volts through it.\nTo increase the conductivity, as you know, you can add some type of electrolyte to the water (like table salt, NaCl).\n\nLet me take a step back right now.\nIf you were to break apart water into pure Hydrogen and Oxygen gas, this only requires a very small voltage, something around 1.5 volts or there abouts (I can look this number up if it is that important to you).  One you have obtained the minimum voltage, it is the current passing through the water the controls the speed of electrolysis.\nAll the voltage over the minimum is called the "over voltage".\n\nWhen you apply a greater voltage than is necesary to the water, you increase the likely hood of reducing/oxidizing things other than water.  Without going into too much detail about the chemistry of it all, you are producing Hydrogen gas at your cathode (-), but at the anode (+), you are probably not producing pure Oxygen, more likely it is Chlorine gas since the Cl- ion is easier to oxidize than the Oxygen in the water.  When you add NaCl to the water, you are only making it easier for it to produce Cl2 gas since it concentration increases.\nThe choice of electrolyte is important as it determines exactly what gasses you will be producing.  In this case, the Cl- ion from the salt is keeping you from making Oxygen gas.  Cl2 gas is very corrosive (not to mention deadly).\n\nThe type of electrode is also very important as some metals will corrode very easily during electrolysis while others are relaitively inert.  Carbon (graphite) and inert metals like platinum, gold and silver (<-- $$$) and popular choices for the anode which is prone to corrosion.  However, for the cathode, you have much greater latitude since the electrode is said to be protected by virture of its charge.\nPersonally, I use carbon-graphite electrodes because of their relative inexpensiveness, however, they do tend to errode over time and need replacing.  When the graphite electodes erode, they leave a fine black powder in suspention in the water which can be filtered out.\n\nLong story short, that slime is most likely the remnants of your electodes corroding away.  Have you noticed you anode betting corroded?\n\nWhat I would do if I were you,\n-switch to graphite electrodes\n-reduce the input voltage in the cell to less than 10 volts (ideally less than 5)\n-use a NaOH electrolye in DI water
976128
I believe the answer is conductive.  This is the process in which things are silver plated.  \n\nHere's how it goes.You fill a tray that has been lined with aluminum foil with salt water ( or is it plain water ? ).  You run a current through the aluminum foil.  The electrons in the the foil get excited due to the electrical current and start releasing aluminum ions ( Al-, I think )  Now, take your rusty, dull ' silver ' spoon.  Place it in the bath for about 2 hours.  Be careful,  electricity, water and living things don't mix well.  After 2 hours, remove the electrical current source and remove the spoon.  The free ions in the water would have coated the spoon, making it shining again.\n\nActually, toothpaste to clean the spoon is easier.
328055
One current method, is called PEM, or proton exchange membrane fuel cells.  How it works:\n\nHydrogen (H2) molecules are split by way of an anode, into protons and electrons.  The membrane allows protons to pass through and blocks electrons.  This creates an electric potential,  as well as a direct current (DC) as collected electrons move around the membrane to the other side, to recombine with the H+ ions (protons) as well as O2 molecules, creating byproducts of water and heat.  This DC could ideally power anything from a light bulb to propelling an automobile if the electricity were converted to mechanical energy (like in the electric motor portion of a hybrid automobile).\n\nThe difficulty comes in getting the hydrogen.  While the byproduct of a hydrogen powered car is water and heat, which do not hurt the atmosphere, the creation of purified hydrogen, does require energy as well as gives off large amounts of CO2, a greenhouse gas.  Some work is being done into looking into renewable energy sources to power the purification process (wind power, solar power, nuclear power, etc) as well as methods of "burying" the produced CO2 underground, so that it is not released into the atmosphere.
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
328575
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.
870424
in electrochemical cells we have chemical reaction . since conversion of this chemical energy to electric energy is mainly becoz of combination of ions ..we hav electric on account of this chemical energy till we have free ions to combine once all ions of solution combines  no more energy conversion is there