I did a lab where we had to determine the iron content in ore...i am confused about the reactions that occured during the reaction...i need reactions for the following...

Question

1) The samples were treated with 6M HCl until all the iron ore dissolved.Assuming all of the ore is in the form Fe2O3m, what is the balanced equation for this process?

What I have is..

Fe2O3(s) + 6HCl (aq) --> 2FeCl3(aq) + 3H2O (l)

2) Samples were then treated with Zn metal according to the following balanced chemical equation...

i have the following, but am unsure if it is correct and if it is i am unsure how to balance it (charges..)

2FeCl3(aq) + 3Zn(s)--> 3ZnCl2(aq) + 2Fe^3+

3) Immediately prior to titration, any excess zinc was removed by treatment with 3M H2SO4 according to the following balanced chemical equation:

I am not sure how to go about writing this equation....

Any help or guidance would be greatly appreciated!!

Answer 1

The 2nd reaction is
2FeCl3(aq) + 3Zn(s)--> 3ZnCl2(aq) + 2Fe(s)
The excess zinc removal reaction is
Zn(s) + H2SO4(aq) --> ZnSO4(aq) + H2(g)