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
The balanced chemical equation for this reaction is: FeS + 2H⁺ → Fe²⁺ + H₂S
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.
Fe2+Cl=FeCl (Original)Fe2+2Cl=2FeCl (Balanced)---- The two in front of the FeCl balances Fe by making it Fe2, but also turns Cl into Cl2. So you put a 2 in front of the Cl reactant, balancing Cl and Fe.
Cu2+(aq) + 2e- → Cu(s) and Fe(s) → Fe2+(aq) + 2e-
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-)
Fe + S = FeS
Zn(s) → Zn2+(aq) + 2e- and Fe3+(aq) + e- → Fe2+(aq)
The chemical formula for iron(II) sulphate is FeSO4, for iron(III) sulfate is Fe2(SO4)3 The formula for iron(II) sulfide is FeS, iron(III) sulfide Fe2S3
Fe(s) + Sn2+(aq) -> Fe2+(aq) + Sn(s)
When an iron nail is dipped in copper sulfate solution, a displacement reaction occurs. The iron nail will displace the copper from the copper sulfate solution to form iron sulfate solution and copper metal deposits on the nail. This reaction is represented by the equation: Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s).