Chemistry help??

Question

Iron metal is recovered from passing carbon monoxide over teh iron ore (Iron III Oxide) forming carbon dioxide and iron metal

Balance teh reaction equation
it would be Fe2O3--->CO+Fe???

When 116 g of CO reacts with excess Fe2O3, how many moles of Iron metal is recovered with a theorectical yield
116 divided by number of moles of Fe2O3 times 100 to get theorectical yield

If the process is not efficient, only 80% yield of Fe is recovered. How many grams would you recover from 116 gm of CO.
116 times 80% to get number of grams

Answer 1

You said that iron is formed by passing CO over iron ore, producing iron and CO2. So the unbalanced reaction is Fe2O3 + CO --> Fe + CO2.

The balanced reaction is Fe2O3 + 3CO --> 2Fe + 3CO2.

A mole of CO weighs 28.009 grams. So 116 grams is 116/28.009 = 4.1415 moles of CO. It takes three moles of CO to produce two moles of iron, so you get 4.1415*2/3 = 2.7610 moles of iron.

If you only get 80% yield, then only 2.7610*0.8 = 2.2088 moles of iron are recovered. A mole of iron weighs 55.845 grams, so the mass of iron recovered is 2.2088 * 55.845 = 123.3512 grams.

Answer 2

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Answer 3

it would be Fe2O3--->CO+Fe??? No...check that your reactants are on the same side! Also you are missing a product!