LEARN MORE...

preparation of a complex iron salt

Anonymous
timer Asked: Jul 7th, 2014
account_balance_wallet $5

Question Description

calculate the number of grams (theoretical yield)of the final iron complex that can be produced from 10.00 g of ferrous ammonium sulfate hexahydrate

Tutor Answer

sobia
School: University of Maryland

the stoic ratio in rxn 2 is 6:2 So first you multiply 0.01202 by 6. Then divide that by 3 to give you the number of moles for Fe(OH)3 + 6H2O which gives you 0.0204 mol. then you use that to find the grams which you dont really need, i think. For the third rxn the ration is now 2;2 or 1:1. So what I did is divide 0.0204 mol by 2 and that gives u the number of moles for the iron complex = 0.0102 mol * 491.1 g/mol which gives a mass of 5.009 g. 

Download Completed Work
flag Report DMCA
Review
Anonymous
Goes above and beyond expectations !

Brown University





1271 Tutors

California Institute of Technology




2131 Tutors

Carnegie Mellon University




982 Tutors

Columbia University





1256 Tutors

Dartmouth University





2113 Tutors

Emory University





2279 Tutors

Harvard University





599 Tutors

Massachusetts Institute of Technology



2319 Tutors

New York University





1645 Tutors

Notre Dam University





1911 Tutors

Oklahoma University





2122 Tutors

Pennsylvania State University





932 Tutors

Princeton University





1211 Tutors

Stanford University





983 Tutors

University of California





1282 Tutors

Oxford University





123 Tutors

Yale University





2325 Tutors