Posted by Sarah H on .
Hi, please check my work:
In an experiment, 23.4 g of FES are added to excess oxygen and 16.5 g of FE2O3 are produced. The balanced equation is:
4FeS + 7O2 --> 2Fe2O3 + 4SO2
Calculate the % yield.
4mol FeS / 0.266 mol = 7mol O2/ x02
mFe2O3 = nXM
= 0.466 mol x 159.7 g/mol
= 74.4 g
% yield = actual yield / theoretical yield X 100%
=16.5 g/74.4 g x 100%
gr. 12 chemistry - drwls, Saturday, May 24, 2008 at 5:08pm
That equation does not look balanced to me. Check the oxygen on both sides.
-this was the balanced equation out of the textbook...i can't believe the textbook's wrong (again)...
grade 12 chem - check my answer again please -
you should get half the moles you started with.
expected yield=.133 moles or .133*molmassFe2O3
= about 77 percent
check that thinking. In your second step you solve for xO2. Why?