veerenyadav
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Reaction in metal oxides and slats
Is there any metal salt which reacts with metal oxide ?
MS+NO ---- MN+NS ?
M = ?
N= ?
S = Cl, Br, etc
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j_sum1
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I think you can answer your own question by considering the stiochiometric ratios in your hypothetical reaction scheme.
What happens to the O in your equation?
How can there be more N in the products than the reactants?
Intermetallics do exist (MN in your equation) but to my knowledge this only occurs when cooling from a melt. Now, I could be wrong. And there is
such a thing as an alloy which occurs at non-specific elemental ratios. But I see no way this could occur from the reaction you describe.
It might be possible to have a displacement reaction involving an oxide an a salt:
MS + NO = MO + NS
I am not aware of any specific examples off the top of my head -- but that could be more to do with the current state of my head than anything else.
In any case, this is quite different from what you have described.
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veerenyadav
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let me correct it
MS+NO ----> MN+NO
for example MnCl2+ XO2 ---> MnO2+XCl2 ?
now is there any X ?
thanks
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veerenyadav
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MS+NO ----> MO+NS
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j_sum1
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Third post asks a sensible question.
Already answered in last paragraph of my previous post.
Someone else may know more.
Aqueous or thermite conditions?
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veerenyadav
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Aqueous system . So it could be M++ , etc
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MrHomeScientist
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If you find a soluble oxide I suppose that could work. The reaction would then be driven by the insolubility of manganese dioxide.
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Melgar
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I'm assuming KMnO4 doesn't count as a metal oxide? I guess one of the issues is solubility. Metal oxides typically aren't water-soluble. If they
are, it's usually because they formed hydroxides instead, and thus are no longer oxides. So the reaction wouldn't be able to progress very quickly,
and would be hampered by insoluble reactants and products.
I did think of an example though. Silver chloride could fit the bill, since it tends to behave more like a covalent substance than an ionic one.
It's barely soluble in water, but can dissolve a little. It also easily splits with halides, forming halogen radicals and metallic silver.
The first step in the process of learning something is admitting that you don't know it already.
I'm givin' the spam shields max power at full warp, but they just dinna have the power! We're gonna have to evacuate to new forum software!
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JJay
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Does barium peroxide count as a metal oxide?
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gdflp
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Thread Moved
27-10-2017 at 08:04 |
Melgar
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Incidentally, if you don't care that the metals are technically hydroxide compounds, but could be formed from oxides, or could form oxides if
dehydrated, then reactions like this would work:
Na2O + AlCl3 = NaCl + Al2O3
Although in reality, it would be:
Na2O + H2O = NaOH
NaOH + AlCl3 = NaCl + Al(OH)3
Al(OH)3 + heat = Al2O3 + H2O (g)
The first step in the process of learning something is admitting that you don't know it already.
I'm givin' the spam shields max power at full warp, but they just dinna have the power! We're gonna have to evacuate to new forum software!
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unionised
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I'm pretty sure that MgS and PbO would react to form PbS and MgO
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