I'm still doing a chemistry page and need help with this question. can someone please explain how to do it...i need a step by step explanation if possible! thank you!
2007-01-05 17:06:32 · 3 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
Do your own homework - But.
Eliminath the 38% contamination
Then workout the ratios of atomic weights for the Fe2O3
Apply the ratio to the 620 kg of ore
Presto. assuming a 100% recovery rate - you may need to adjust.
2007-01-05 17:16:14 · answer #1 · answered by ch33tah2011 2 · 0⤊ 0⤋
calculate how much fe2o3 can be extracted frm 1000 kg of ore
ie 630 kg
now from fe2so3 55.8*2 gm(molar mass of fe) of fe could be extracted
159 .6 gm of fe2o3(molar mass of fe2o3)====>111.6gm of fe
1gm=====>111.6/159.6
630kg======>(111.6/159.6)*630
=440.5 kg
2007-01-05 17:21:25 · answer #2 · answered by miinii 3 · 0⤊ 0⤋
% by mass of Fe2O3 = (mass of pure Fe2O3 / mass of iron ore) x 100% mass of Fe2O3 (pure) = (mass of iron produced / MW of iron) x ( stoichiometric mole ratio of Fe2O3 over Fe based on the given chemical reaction x MW of Fe2O3 mass of iron produced = 453 g MW of Fe = 55.85 stoichiometric mole ratio of Fe2O3/Fe = 1/2 MW of Fe2O3 = 159.7 mass of pure Fe2O3 = (453/55.85) x (1/2) x 159.7 mass of pure Fe2O3 = 647.66 grams %by mass of Fe2O3 = (647.66 / 752) x 100 = 86.13 %
2016-05-22 22:05:19 · answer #3 · answered by Anonymous · 0⤊ 0⤋