What type of chemical reaction is this? I2O5 + 5CO → I2 + 5CO2?
Hi! I have this chemical reaction:
I2O5 + 5CO → I2 + 5CO2
diiodide pentoxide + carbon monoxide → iodine + carbon dioxide
I'm trying to figure out if this reaction is a single replacement, double replacement, or something else. I'm leaning towards double replacement... but why and how does iodine end up by itself? Then, would it be a single replacement?
Any help would be much appreciated! Thank you!
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Reaction type....
Not all chemical reactions fit these common reaction types taught in first-year chemistry: synthesis, decomposition, single replacement, double replacement and the complete combustion of a hydrocarbon. Each has its own distinctive pattern, and the question you have given does not fit any of those. Indeed there are lots of reactions which won't fit those patterns.
It has been said that it is a redox reaction (oxidation-reduction*). That is not a separate reaction type, it is merely a way to describe some reactions. For instance, all single replacement reactions are redox, so is the complete combustion of a hydrocarbon. Some synthesis and decomposition reactions are redox. What you would almost never see are double replacement reactions being redox. Therefore, it is obvious that "redox reaction" is not a "type" of reaction so much as just a description which can be applied to several different types of reactions.
2H2(g) + O2(g) --> 2H2O(g) ............ ......... synthesis and redox
2SO3(g) --> 2SO2(g) + O2(g) .......... ......... decomposition and redox
Zn(s) + 2HCl(aq) --> ZnCl2(aq) + H2(g) ..... single replacement and redox
CH4(g) + 2O2(g) --> CO2(g) + 2H2O(g) ..... complete combustion of a hydrocarbon and redox
Oxidation == increase in oxidation state
Reduction == decrease in oxidation state
+5-2........ +2-2 ......... 0 ........ +4-2 ........... oxidation states
I2O5(s) + 5CO(g) --> I2(s) + 5CO2(g)
Iodine is reduced, carbon is oxidized
It is an oxidation-reduction reaction, and the way you can tell is to look and see if any of the elements have changed oxidation state. In this example, I on the left (in I2O5) has an oxidation number of 5+ and on the right it is zero. So, it has been reduced. The oxidation number of C on the left (in CO) is 2+ and on the right (in CO2) it is 4+. So it has been oxidized.
It is an oxidation-reduction reaction.