Iron+dilute sulphric acid?

Iron can react to form iron(II) or iron(III) compounds. When iron reacts with substances which are NOT oxidizing agents, iron(II) compounds are formed. When iron reacts with substances which are oxidizing agents, iron(III) compounds are formed.

When iron reacts with an acid, the type of reaction depends on whether the acid is an oxidizing agent or not.

When iron reacts with an acid which is NOT an oxidizing agents, iron(II) salt and hydrogen are formed.
Fe + non-oxidizing acid → iron(II) salt + hydrogen
Common examples include:
Fe + H2SO4(dil.) → FeSO4 + H2
Fe + 2HCl(dil./conc.) → FeCl2 + H2
Fe + 2CH3COOH(dil./conc.) → (CH3­COO)2Fe + H2

When iron reacts with an acid which is an oxidizing agent, redox reaction occurs. The products include iron(III) compound(s), but NO hydrogen will be formed. Common examples include:
2Fe + 6H2SO4(conc. and hot) → Fe2(SO4)3 + 6H2O + 3SO2
Fe + 6HNO3(conc.) → Fe(NO3)3 + 3H2O + 3NO2
Fe + 4HNO3(dil.) → Fe(NO3)3 + 2H2­O + NO

Iron can become Iron(II) ion in FeSO4 or Iron(III) ion in Fe2(SO4)3.

but for the dilute acid, it is more likely to have more FeSO4 since the oxidizing power of dilute acid is weaker.

Metal + Acid -> Salt + Hydrogen

Iron(III) + Dilute sulphric acid -> Salt + hydrogen

Fe(s) + H2S04(aq) -> Fe2(SO4)3(s) + H2(l)