How to balance chem.eq. with crystal water?

[eventob]

1. The problem statement, all variables and given/known data
10 g Fe and x ml H2SO4 forms y gFeSO4*7H2O

Write a balanced chemical equation for the reaction, and determine the coeffisients y and x. The H2SO4 is 1 M.


2. Relevant equations
n=V*c
n=m/Fm


3. The attempt at a solution
First thing I was trying to set up the chemical eq:
Fe+H2SO4 => FeSO4*7H2O

But, I'm not sure how to balance the hydrogens and oxygens in the crystal water.

I've also calculated the how many moles 10 g of Fe is.


Any thoughts?

Thanks in advance.

[Borek]

You need to add water molecules on the left - after all, reaction takes place in a solution. If not, there is no way hydrated salt can be produced.

[eventob]

Thanks.

But then, do I have to add hydrogen to the right?

Fe+H2SO4 + 7H2O => FeSO4*7H2O + H^+

[Borek]

Other than water of crystallization it is not different from the reaction between a metal and an acid. I am more than sure that you have covered this reaction earlier, so check your notes and the book. Googling for reaction between metal and acid will also give you the answer.

[eventob]

Thanks again. :)

I tried to Google it first, but could only find formulas without the crystallization water. So I was not sure how to handle that part. I am currently taking two different chemistry courses, one introductory and one who builds one the knowledge from the introductory course. I've never seen the *H2O part until this reaction. :)

[symbolipoint]

Writing a balanced reaction should be no big problem. Look at the mole ratios among the parts and the materials. Post #3 reaction is almost, but not yet balanced. No matter, you can still write enough reaction without including the H+ ions.

Use given information and formula weights to account for both grams and moles.
10 grams Fe ----- How many moles?
1 to 1 mole ratio of Fe to FeSO4*7H2O ----- then how many moles and how many grams if starting from 10 grams of Fe ?