Question

Ia a iron(III) and copper (II) solution what is the following?
what are the reactants, the predictiono reaction type what is the reaction type!
Detail:Iron (IIII) and copper (II) sulfate solution
Fill a small test tube halfway with copper (II) sulfate solution. Add a 2.0 gram iron rod to the solution and observe the reaction.
the observcation is that th iron to the solutionit turned like red ish like lava color or something!

Answer 1

please i really need help with it i'm stock!!

Answer 2

You're working with ionic compounds dissolved in solution, so the species that might react are all ions. What kind of chemical reactions can ions undergo? Only two are common: precipitation reactions, in which cations and anions get together to form a new ionic solid, or redox reactions, in which ions exchange electrons and change their charges.

For example, if you had Ag+ cations and Cl- anions in solution, they would naturally get together to form solid AgCl. That's an example of a precipitation reaction.

On the other hand, if you had Fe+3 ions and Cu+ ions in solution, they could exchange electrons. An electron could leave the Cu+ ion, turning it into a Cu+2 ion, and join the Fe+3 ion, turning it into a Fe+2 ion. That's an example of a redox reaction. ("Reduction-oxidation" where "reduction" = gain of electrons, and "oxidation" = loss of electrons.)

Now let's apply these general ideas to your particular problem. You've got several metals, both in solution and in the solid form (as the iron rod), and one anion, the sulfate (SO4-2) anion. Precipitation reactions aren't going to happen, because sulfates in general are soluble, except with lead, mercury and barium cations -- none of which you have here.

So you're looking at whether a redox reaction is possible. One limitation on redox reactions is that the reactant *and* product ions must be stable, so you need atoms with more than one stable oxidation state (e.g. charge in solution). Only metals fit that bill, generally, and the various metals have quite specific possibilities. There are some patterns, but most often students just memorize the various charges possible for the more common metals.

In this case, you have copper and iron, and copper cations are stable as either Cu+ or Cu+2, while iron cations are stable as either Fe+2 or Fe+3. Of course, both metals are also stable as the pure metal, Cu or Fe. So those are the possible reactants and products.

Now, you're beginning with pure iron (the iron rod), Fe, plus copper (II) sulfate solution, which means Cu+2 in solution. You're told a reaction occurs, because something about the solution changes -- its color in this case.

What could happen? Look at your possible reactants and products: Fe could be turning into Fe+2 or Fe+3, while the Cu+2 could be turning into Cu+ or Cu. Either way, you can see the Fe would be losing electrons (being oxidized) and the Cu would be gaining electrons (being reduced).

So tentatively we would say the redox reactions that could be going on would be:

Fe(s) + Cu+2(aq) -> Fe+2(aq) + Cu(s)
Fe(s) + 2 Cu+2(aq) -> Fe+2(aq) + 2 Cu+(aq)
2 Fe(s) +3 Cu+2(aq) -> 2 Fe+3(aq) + 3 Cu(s)
Fe(s) + 3 Cu+2(aq) -> Fe+3(aq) + 3 Cu+(aq)

How did I balance those reactions? By taking careful note of the electrons released and absorbed on each side. For example, in the first case, to go from Fe to Fe+2 releases two electrons, which are absorbed by the Cu+2 going to Cu. In the second case, the Cu+2 going to Cu+ only absorbs one electron, so I need two Cu+2's to absorb the two electrons released by the Fe going to the Fe+2. And so on.

We've actually gotten pretty far already. We've identified the likely reaction as a redox reaction, we've seen that clearly the iron must be oxidized and the copper reduced, and we've written balanced net ionic reactions for the four possible redox reactions.

The only remaining question is which of these reactions it is. The only clue we're given is that the solution turns red, or that there's a red coating on the iron (not sure which you mean). That suggests the presence of the Fe+3 cation, because that cation is reddish (it gives the color to rust and blood). That suggests one of the last two reactions, which have Fe+3 as a product. A more sophisticated point of view takes note of the fact that Cu+ is very easily reduced to Cu, so that a product of Cu+ under these conditions is a little unlikely (it would just go on to be reduced to Cu). That leaves the third reaction as the most likely:

2 Fe(s) +3 Cu+2(aq) -> 2 Fe+3(aq) + 3 Cu(s)

In this reaction, the iron is oxidized to the ferric or iron(III) cation, and the cupric or copper(II) cation is reduced to copper.

Answer 3

it is just displacement reaction!!!
one metal displaces other metal duet change in their electrode chemical potential.
if you compare the electrode potential values it will tell the reaction type!!!
The featoms has tendency to lose electron and get converted into ions where as copper has tendency to get reduced to copper metal !!!!as result you are watching brown ppt which is nothing but copper metal !!!!!
Fe-0.044 -ve indicates tendency to lose electron
Cu+0.34 + ve indicates tendency to gain electron in these case!!!!!