Fe2O3 + H2 --> Fe + H2O A) what mass of hydrogen gas must be consumed to produe 10.0 g of iron metal? B) what mass of iron(lll) oxide, Fe2O3, must be consumed to prepare 2.50…

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asked Dec 3, 2016 204k views

1 Answer

Darren Corbett · Answer 1 · 2016-12-07T00:45:03+0000

A) 10.0g of Iron is
(10.0)/(55.8)=179mmol

of Iron.

One mole of dihydrogen is required to form one mole of iron, hence you'll need
0.179*1.00=0.179g

of dihydrogen.

B) Likewise : 2.50g of Iron is
(2.50)/(55.8)=44.8mmol

of Iron, hence we'll need
44.8*(3*16+2*55.8)=7.15g

of Fe2O3.