the reaction equation is in moles
so you need to convert grams of iron oxide to moles
the molar mass is 159.7 (two iron plus 3 oxygen)
14.7 g / 159.7 g/mol = .092 moles
the reaction equation shows 3 moles of carbon dioxide for each mole of iron oxide
so .092 * 3 = .276 moles of CO₂
the molar mass of CO₂ is 44.0 g
a) .276 * 44.0 = 12.1 g
the percent yield is the actual amount divided by the theoretical amount
b) 8.73 g / 12.1 g = .721 = 72.1%
Iron can be produced by the reduction of iron(III) Oxide by carbon monoxide:
Fe2O3 + 3CO -> 2FE +3CO2
a) what maximum mass of CO2 could be produced from the complete reduction of 14.7g of Fe2O3?
b) if 8.73g of CO2 gas was actually collected, what percentage yield of the reaction?
can you please go into detail i cant seem to understand it no matter how many people show me the work on how they do it.They all seem to do it differently and i just can't seem to get it.
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