Cobalt, which forms CO2+ ions will displace tin from its salt tin(II) chloride, SnCl2.
What would you expect to observe as this reaction proceeds?
What would you expect to observe if you placed cobalt chloride solution in a tin can?
Since we have tin(II) the chlorine must be in the state Cl-. So we will form CoCl2. This should be a precipitate, but I'm not completely sure of this. (And if the whole reaction is done in an aqueous solution I'm not too sure we wouldn't be producing HCl instead of the CoCl2. I'm probably being too careful in suggesting this, but it would be something to check out.)
Since the Co will replace the Sn in the above reaction, the CoCl2 should be stable when placed in a tin can. (There will be some slight erosion of the tin due to the reverse reaction, but since the reaction prefers to go forward I would think this erosion would be slight.)
Hi topsquark, yeah CoCl2 is aq and does not precipitate
Co(s) + SnCl2(aq) → Sn(s) +CoCl2(aq)
Co(s) + Sn2+(aq) → Co2+(aq) + Sn(s)
How do I write the balanced equation for
Zinc is added to nitric acid to produce Zn2+ ions and nitrous oxide, N2O (laughing gas)
An aqueous solution of iron(II) ions is oxidised to iron(III) by an acidified solution of dichromate ions, Cr2O72-