electrolysis chemistry
136150
I don't know of a solution that will color copper blue, but sulfuric acid will attack copper and produce a blue solution of copper sulfate.
215740
1) FIND THE REDOX-REACTION\n\nChromate (+VI) is reduced to 2 Cr(III) meaning this that 6 electrons are needed.\n\nThe corresponding oxidation on the alpha-C-atom in Ethanol goes from oxidation-level (-I) to oxidation-level (+III) in acetic acid, meaning it delivers 4 electrons per molecule.\n\nSo we find a stochiometric electron equilibrium if 12 electrons are exchanged:\n\n2 Cr2O7(2-) + 3 CH3CH2OH  =  4 Cr(3+) + 3 CH3COOH\n\n2) THE PROCESS MUST BE ELECTRICALLY NEUTRAL\n\nWe add the K-Ions having the left side of the equation neutral and the right side with 16 loads positive:\n\n2 K2Cr2O7 + 3 CH3CH2OH  = 4 Cr(3+) + 4 K(+) + 3 CH3COOH\n\nIn order to have the left side also with 16 loads positive, we add 16 protons, meaning this, that the reaction needs acid. Since we use sulfuric acid we also add 8 sulfat-ions on both sides and hereby can neutralize the product side:\n\n2 K2Cr2O7 + 8 H2SO4 + 3 CH3CH2OH  =\n                         2 Cr2(SO4)3 + 2 K2SO4 + 3 CH3COOH\n\n3) STOCHIOMETRIC BALANCE OF THE ELEMENTS H and O\n\nTaking into consideration that unused protons finally end up as water, we add on the right side 11 H2O and hereby is also reached the balance of oxigen:\n\n2 K2Cr2O7 + 8 H2SO4 + 3 CH3CH2OH  =\n                  2 Cr2(SO4)3 + 2 K2SO4 + 3 CH3COOH + 11 H2O\n\nSo now good luck for counting the atoms!
555426
You could use the batteries to electrolyse brine (ordinary table salt dissolved in water), causing chlorine and hydrogen gas to build up. If you could contain the hydrogen and chlorine somehow and let it build up to high pressure, you could let the pressure propel the rocket, or (if you allow air/oxygen in somehow) you could ignite the hydrogen.\n\nTry searching electrolysis on google for more info if you don't know what I'm talking about.
239401
During electrolysis, the oxygen atom in H20 has 2 pairs of unbonded electrons, and it is these electrons that act as "solvents" breaking the bond between atoms and attacking the postive ion that forms as a result.  So you can visualize a solution as islands of ions surrounded by water ions, with the extra electrons of oxygen surrounding the positive ions and the negative ions surrounded by the hydrogens of water.  \n\nA "strong" electrolyte is one that dissociates almost completely into ions i.e the water molecules break its bond and surround its ions easily.  HCl is a good example.  HF is an exception.  Since F is the element with the strongest electronegativity (4.0) it forms very strong bonds.  And, apparently, water molecules just don't have the ability to break the H-F bond, so very little of HF ionizes in water.    Talking about HF, it is one of the few compounds (and as far as I know, the only compound) that can attack glass (Si03) to form fluorosilicates.
319335
1.) do your own homework\n2.) this is the computer forum, not high-school chemistry.  Next time post to the right furom.
167911
go to\nwww.chemistry.com
526890
http://www.chemguide.co.uk/physical/catalysis/hydrolyse.html   \n                                                                                                    this will help ya
484918
44 A) 2AgO --> 4Ag + O2\n     B)NiCO3 --> NiO + CO2\n     C)NH4NO3 --> N2O + 2H2O\n48)A)2HCl + Ca(OH)2 --> CaCl2 + 2H2O\n     B)3Ag2SO4 + 2AlCl3--> 6AgCl + Al2(SO4)3\n     C)&D) I've no idea, sry\n50)A)C4H8 + 6O2 --> 4CO2 + 4H2O\n     B)2C8H18 + 25O2 --> 16CO2 + 18H2O\n     C)2C3H8O3 + 7O2 --> 6CO2 + 8H2O\n     D)2C3H6O + 5O2 --> 6CO2 + 6H2O\n52)A)2Al + 3H2SO4 --> Al2(SO4)3 + 3H2\n     B)2HCl + Ba(OH)2--> BaCl2 + 2H2O\n     C)Au + HCl--> No Reaction(gold is below hydrogen in the metal reactivity series)\n54)A)2Cl2 + 2NaI --> 2NaCl2 + I2\n     B)2NH3--> N2 + 3H2\n     C)4Na + O2--> 2Na2O\n     D)Mg + H2SO4--> MgSO4 + H2\n     E)MgCl2 + Ca(OH)2--> Mg(OH)2 + CaCl2\n     F)H2 + Cl2--> 2HCl
139605
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.
281072
I agree with the first poster on C and E, but I'm not sure if A is also.  A solute dissolving in a solvent seems like a chemical process to me, but I don't remember for sure.
394493
For aA+bB -> cC+dD\n\nE=E0-(RT/nF)* ln([C]^c*[D]^d / ([A]^a*[B]^b))\n\nwhere n=number of electrons taking part in the reaction\n\nSolids are not considered in the equation, so in your case\n\nE=E0 -(RT/nF)*ln([Fe2+]/[Cd+2])\n\nYou can find the standard reduction potentials for the Fe+2 and Cd+2 at \nhttp://www.northland.cc.mn.us/Chemistry/standard_reduction_potentials.htm\nThen E0= E0(Cd2+)-E0(Fe2+)\nR=8.314\nn=2\nF=96500\n\nYou have to specify T ...
551243
I assume that you mean that the resistance of the solution kkeps rising with time. If you are using a Dc based system, then depending on the conductivity (1 over the resistance) electrolysis products may be building up at the electrodes and increasing the resistance. A yourself a good conductivity meter and this should eliminate the problem.\n\nThe resistance of a solution will dpend on the area of your electrodes, the distance bewteen them ,the concentration of dissolved salts in the water and the solution temperature. You will have a few things you will need to keep standard.
475180
In B, oxygen is a waste product of photosynthesis, but oxygen can also be produced in D. In electrolytic cells the electrolysis of salt water or acidic water is an  example of electrolysis. The ionic solution is driven by current and produces hydrogen gas in a reduction reaction at the cathode using electrons to complete the hydrogen ions. At the anode OXYGEN gas is produced in an oxidizing reaction and electrons are given off as the oxygen ions combine.
595953
Gee, I know you're a student but you are dull and lazy.\n\nHaven't you heard of google??  \n\nStep 1 - I went to www.google.com\nStep 2 - I used the following search  "electroclorination +equation"\n\nhttp://www.google.com/search?hl=en&lr=&q=electrochlorination+%2Bequation\n\nStep 3 - I followed the first link (listed below) on the google.com search results.\n\nAnd you've waited how many days for this answer?  It took me less than one minute to find.
345703
Hi,\nHere you can find a table:\n\nhttp://www.physchem.co.za/Data/Electrode%20Potentials.htm
473792
these electrons are the ones that participate in chemical reactions, ie formation of bonds
105188
In the case of metals what happens is that the protons "steal" the electrons of the metal to evolve a H2, or hydrogen gas, in doing so, the metal for example Fe, turns to Fe++ which will dissolve, if the acid used is HCL then you'll get as products H2  and Iron Chloride, if the acid is sulfuric, you'll get H2 and Iron Sulfate. This is completely electrochemical, whereas when an acid attacks  cement is just chemical, and what evolves is carbon dioxide, with skin, I'm not so sure.