We have this 32 problem worksheet on stoicheometry the sub couldn‘t even help us.1) The process reducing iron ore into solid iron metal solid iron (III) oxide is reacted with gaseous carbon monoxide in order to form gaseous carbon monoxide and iron metal. balancea)What is the maximum mass of iron, in grams, that can be obtained from 454 grams of iron (ii) oxide?b)What mass of carbon monoxide is required to reduce the iron (ii) oxide to iron metal?
I think there is a mistake in this statement The process reducing iron ore into solid iron metal solid iron (III) oxide is reacted with gaseous carbon monoxide in order to form gaseous carbon monoxide and iron metal. balance. You can't react iron oxide with carbon monoxide and get iron and carbon monoxide, I think it should read The process reducing iron ore into solid iron metal solid iron (III) oxide is reacted with gaseous carbon monoxide in order to form gaseous carbon dioxide and iron metal Fe2O3 + CO - Fe + CO2 From the problem, the iron oxide is given as Fe(III). Since O is -2, you need two Fe(III) and three O -2 in the compound. Balancing the reaction gives you Fe2O3 + 3CO - Fe + 3CO2 Fe2O3 has a molecular weight of 159.7 g / mole. 454 g 2.84 moles. From the equation, you make the same number of moles of Fe, 2.84. The atomic mass of Fe is 55.85 so the mass of Fe is 55.85 g / mole * 2.84 moles 158.8 g For every mole of Fe2O3, you need 3 moles of CO so you need 2.84 moles * 3 8.52 moles. The molecular weight of CO is 28.01 g / mole so you need 8.52 moles * 28.01 g / mole 238.6 g
There is no point. Yes it could be done, but the vehicle structurally will probably not be able to handle it.
