(a(i))[1]
Write a balanced equation for how the iron in the wire reacts with the sulfuric acid.
(a(ii))[1]
Use the half-equations to form an equation for the reaction between the iron(II) ions and the acidified dichromate(VI) ions.
(a(iii))[1]
Calculate the amount, in moles, of dichromate(VI) ions used in the titration.
(a(iv))[1]
Calculate the amount, in moles, of iron(II) ions in the $25.0\,\text{cm}^3$ sample of solution.
(a(v))[1]
Calculate the amount, in moles, of iron in the $3.35\,\text{g}$ piece of wire.
(a(vi))[1]
Calculate the mass of iron in the $3.35\,\text{g}$ piece of wire.
(a(vii))[1]
Calculate the percentage of iron in the iron wire.
(b(i))[2]
Use the data to suggest the nature of the bonding in iron(III) chloride. Explain your answer.
(b(ii))[1]
Suggest an equation for the reaction of iron(III) chloride with water.