veerenyadav - 26-10-2017 at 23:14
Is there any metal salt which reacts with metal oxide ?
MS+NO ---- MN+NS ?
M = ?
N= ?
S = Cl, Br, etc
j_sum1 - 27-10-2017 at 00:33
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.
let me correct it
veerenyadav - 27-10-2017 at 01:01
MS+NO ----> MN+NO
for example MnCl2+ XO2 ---> MnO2+XCl2 ?
now is there any X ?
thanks
veerenyadav - 27-10-2017 at 01:02
MS+NO ----> MO+NS
j_sum1 - 27-10-2017 at 01:35
Third post asks a sensible question.
Already answered in last paragraph of my previous post.
Someone else may know more.
Aqueous or thermite conditions?
veerenyadav - 27-10-2017 at 05:33
Aqueous system . So it could be M++ , etc
MrHomeScientist - 27-10-2017 at 06:11
If you find a soluble oxide I suppose that could work. The reaction would then be driven by the insolubility of manganese dioxide.
Melgar - 27-10-2017 at 06:38
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.
JJay - 27-10-2017 at 07:08
Does barium peroxide count as a metal oxide?
Melgar - 28-10-2017 at 04:22
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)
unionised - 28-10-2017 at 04:26
I'm pretty sure that MgS and PbO would react to form PbS and MgO