Question

What mass of CO is needed to react completely with 55.0 g of Fe2O3 in the reaction: Fe2O3(s) + CO(g) → Fe(s) + CO2(g)? (4 points)

Answer 1

Answer:

Answer:- 28.9 grams of CO are needed to react with 55.0 grams of Iron(II)oxide.

Answer 2

The mass of CO needed to react completely with 55.0 g of Fe₂O₃ is 28.896g.

Given:

Fe₂O₃(s) + CO(g) → Fe(s) + CO₂(g)

To Find:

The mass of CO is needed to react completely with 55.0 g of Fe₂O₃.

Solution:

To find the mass of CO needed to react completely with 55.0 g of Fe₂O₃ we will follow the following steps:

The formula mass of Fe₂O₃ = 159.69 g/mole

The molecular mass of CO = 28 g/mole

The balanced equation is:

Fe₂O₃(s) + 3CO(g) → 2Fe(s) + 3CO₂(g)

Now,

1 mole of Fe₂O₃ reacts with 3 moles of CO.

Moles of 55 g of Fe₂O₃ =

$\frac{given \: mass}{molecular \: mass} = \frac{55}{159.69} = 0.344$

0.344 moles of Fe₂O₃ reacts with (0.344 × 3) moles of CO.

Mass of CO reacted with 55 g of Fe₂O₃ =

$moles \times molecular \: mass = 0.344 \times 3\times 28 =28.896 g$

Henceforth, the mass of CO needed to react completely with 55.0 g of Fe₂O₃ is 28.896g.

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