In laboratory settings, you can make react a mixture of powdered sulphur
and iron filings by heating. The end product is Ferrous Sulfide;
Fe + S ----> FeS
Iron sulfides in nature are Pyrite and Marcasitewhose formula is; FeS2 .
This reaction is:S + 6 HNO3 = H2SO4 + 2 H2O + 6 NO2
Water molecules, H2O have hydrogen bonding between molecules which means it is a liquid until 100 oC, 212 oF. Carbon tetra chloride/ tetrachloro methane is heavy but boils at 76.8 oC
So far I come up with: HBr (aq) + MgSO3 (s) --> H2SO3 (aq) + MgBr2 (??)
3 mole FeCl2 will react with 6 mole NaOH (stoechiometric mole ratio: 1 FeCl2 to 2 NaOH), so 3 mole FeCl2 (= 6 added -3 used) will be left over.
-2.37 V (apex) Chace
A. Fe^2+ ==> Fe^3+ + e- is an oxidation reactionB. Fe^3+ +e- ==> Fe^2+ is a reduction reactionC. Fe(s) ==> Fe(l) is neither an oxidation nor a reduction reaction. It is a phase change.D. Fe + 2e- ==> Fe^2+ is not a possible reaction.
Fe + S = FeS or 2Fe +3S = Fe2 +S3
1/2 Equations Cu2+(aq) + 2e- --> Cu(s) Fe(s) -->Fe2+(aq) + 2e- Overall Equation Fe(s) + Cu2+(aq) --> Cu(s) + Fe2+(aq)
Fe + S = FeS
The oxidation half-reaction is: Fe => Fe+3 + 3e-, and the reduction half-reaction is: F2 + 2e- => 2 F-1. For a complete equation, the oxidation half-reaction as written must be multiplied by 2 and added to the reduction half-reaction as written multiplied by 3 to result in an overall reaction of 2 Fe + 3 F2 = 2 FeF3.
Fe(s) + Cu2+(aq) --> Fe2+(aq) + Cu(s)
Cu2+(aq) + 2e- → Cu(s) and Fe(s) → Fe2+(aq) + 2e-
Zn(s) → Zn2+(aq) + 2e- and Fe3+(aq) + e- → Fe2+(aq)
This is a redox question. In order for Mg2+ to oxidize Fe(s), Mg2+ needs to have a higher reduction potential (tendency to be reduced) than Fe2+. Mg2+ + 2 e− --> Mg(s) E° = −2.372 Volts Fe2+ + 2 e− --> Fe(s) E° = −0.44 Volts (More favorable reaction) Fe2+ has a higher reduction potential than Mg2+, so Mg+2 will not oxidize Fe(s).
When your paper clip is made of (or coated with) more reactive metals than copper, like Fe, Zn or Sn, it might react with Cu2+ ions in your solution. Cu2+ + Fe(s) --> Cu(s) + Fe2+
molecular equation: CuSO4 (aq)+Fe (s) --> Cu(s) + FeSO4(aq) net ionic equation: Cu2+(aq) + Fe2+ (s) --> Cu2+(s) + Fe2+(aq) spectator ion: Sulfate Ion (SO42-)
2 Fe (s) + 3 H 2SO 4 (aq) β Fe 2(SO 4) 3 (s) + 3 H 2 (g). This is an oxidation-reduction (redox) reaction: 6 H I + 6 e - β 6 H 0 (reduction).