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#01 Electrolysis Of Sodium Chloride (Cl2 is produced!) By bla287 When electrolysing a solution of NaCl, you'd normally expect water to be oxidized to oxygen and oxonium because of the electrode potentials: Cl2 + 2 e− ⇌ 2 Cl− +1,36 V O2 + 4 H3O+ + 4 e− ⇌ 6 H2O +1,23 V Nevertheless, you can "trick out" the potentials by using a graphite anode and a saturated NaCl solution. The smaller chloride ion can attach to the graphite more easily than the bigger H2O molecule, so the chloride ion will be oxidized to chlorine ("over voltage" effect). However, some of the chlorine produced that way will react with the OH- ions produced by the cathode to form ClO- and Cl- (in succession ClO3- and ClO4- as well), but not all of it, so you can collect some of the chlorine. To reduce such disproportionation effects, HCl can be added. To prove that chlorine has really been produced, I let it react with iron to form yellow iron(III) chloride (FeCl3). So you don't need to melt NaCl if you want to obtain Cl2 (but you have to if you want to get Na). BTW the gas bubbling up from the metal cathode is hydrogen (H2). Here's a very informative site about (per)chlorate cells: http://www.geocities.com/CapeCanavera... Tags: chlor, chloride, chlorine, cl2, eisen, electrolysis, fecl3, hydrogen, iron, na, nacl, natrium, sodium 1 Downloads - Last from: (Your Blog here!) |
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