Draeger
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Electrolysis of NaCl with Fe - what are the side products?
Since I don't know anything about electrolysis, I am wondering which side products would be made while doing the electrolysis of NaCl solution with
Fe, since I am worried that it would produce chlorine, since I can only do this in a closed space.
Collected elements:
Al, Cu, Ga, C (coal), S, Zn, Na
Collected compounds:
Inorganic:
NaOH; NaHCO3; MnCl2; MnCO3; CuSO4; FeSO4; aq. 30-33% HCl; aq. NaClO; aq. 9,5% ammonia; aq. 94-96% H2SO4; aq. 3% H2O2
Organic:
citric acid, sodium acetate, sodium citrate, petroleum, mineral oil
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subskune
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iron as electrode or as salt in solution?
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Draeger
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Oh. Forgot to state it. As electrode.
Collected elements:
Al, Cu, Ga, C (coal), S, Zn, Na
Collected compounds:
Inorganic:
NaOH; NaHCO3; MnCl2; MnCO3; CuSO4; FeSO4; aq. 30-33% HCl; aq. NaClO; aq. 9,5% ammonia; aq. 94-96% H2SO4; aq. 3% H2O2
Organic:
citric acid, sodium acetate, sodium citrate, petroleum, mineral oil
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Alpine2048
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Are you using iron as both the anode and cathode? And what voltage and current are you running the cell under. Different voltages prompt different
reactions to be favourable.
I would say you are likely going to produce some Fe2O3 in any case if the iron isn't stainless.
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subskune
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On the cathode h2 is produced and the iron will work fine there. On the anode the iron oxidizes instead of chlorine and probably forms some iron
chloride.
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Draeger
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Quote: Originally posted by Alpine2048  | Are you using iron as both the anode and cathode? And what voltage and current are you running the cell under. Different voltages prompt different
reactions to be favourable.
I would say you are likely going to produce some Fe2O3 in any case if the iron isn't stainless. |
Both cathode and anode. And I am running at only 1.5V since that's what a battery can do. I'm not sure that low voltage actually works out, though.
It's just what I have most available.
I want it to produce Fe2O3.
Collected elements:
Al, Cu, Ga, C (coal), S, Zn, Na
Collected compounds:
Inorganic:
NaOH; NaHCO3; MnCl2; MnCO3; CuSO4; FeSO4; aq. 30-33% HCl; aq. NaClO; aq. 9,5% ammonia; aq. 94-96% H2SO4; aq. 3% H2O2
Organic:
citric acid, sodium acetate, sodium citrate, petroleum, mineral oil
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|
|
subskune
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if it is a one pot reaction that might actually work as the hydroxide from the cathode crushes out the chloride at the anode and in the end there will
be some iron oxy-hydroxide mixture.
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Draeger
Hazard to Others
Posts: 185
Registered: 31-1-2020
Location: North-Rhine Westfalia, Germany
Member Is Offline
Mood: Slowly getting ready for new projects
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| Quote: Originally posted by subskune | | On the cathode h2 is produced and the iron will work fine there. On the anode the iron oxidizes instead of chlorine and probably forms some iron
chloride. |
Ah. Thanks.
Collected elements:
Al, Cu, Ga, C (coal), S, Zn, Na
Collected compounds:
Inorganic:
NaOH; NaHCO3; MnCl2; MnCO3; CuSO4; FeSO4; aq. 30-33% HCl; aq. NaClO; aq. 9,5% ammonia; aq. 94-96% H2SO4; aq. 3% H2O2
Organic:
citric acid, sodium acetate, sodium citrate, petroleum, mineral oil
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