# Chemistry

posted by .

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...

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!!

• Chemistry -

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)

## Similar Questions

1. ### chemistry

A 46.9 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 11.6 grams. What was the percent iron in the sample of ore?

A 36.5 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 10 grams. What was the percent iron in the sample of ore?
3. ### chemistry

A 28.6 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 10.1 grams. What was the percent iron in the sample of ore?
4. ### ap chemistry

A 25.2 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 12 grams. What was the percent iron in the sample of ore?
5. ### Chemistry

I have 3 I don't understand how to do. A 33.2 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 12.3 grams. What was the percent …
6. ### AP Chemistry

A 40.3 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 10.5 grams. What was the percent iron in the sample of ore?
7. ### AP Chemistry

A 44.6 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 10.1 grams. What was the percent iron in the sample of ore?
8. ### Chemistry

7) 14 carat gold has a purity of 58.3%. How many moles of gold are in 163 grams of 14 carat gold?
9. ### AP Chemistry

A 33.8 g sample of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 20.7 g. What was the mass of iron in the sample of ore?
10. ### Chemistry

A 39 g of iron ore is treated as follows. The iron in the sample is all converted by a series of chemical reactions to Fe2O3. The mass of Fe2O3 is measured to be 7.9 grams. What was the percent iron in the sample of ore?

More Similar Questions