Q23 Stoichiometry
4 Points
Use the balanced equation: Fe2O3(s) + 3H2(g) →2Fe(s) + 3H2O(l), to answer
following question.
Calculate how many grams of iron metal are produced starting with 0.85 g of Fe2O3 and
excess hydrogen gas. Give your final answer with the correct sig figs and units in the space
below.
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quimbap quimbap · Answer 1 · 2020-05-14T05:37:43+02:00

Answer:

6.0 x 10^-1 g Fe

Explanation:

I might be in the wrong but hear me out:

Convert 0.85 g to mols of Fe2O3.

0.85 g x 1 mol/159.69=0.0053 mols Fe2O3.

Get moles of Fe (iron metal).

0.0053 mols Fe2O3 x 2 mol Fe/ 1 mol Fe2O3

= 1.0 x 10^-2 mols Fe

Convert moles to grams of Fe.

1.0 x 10^-2 mols of Fe x 55.85 grams Fe/ 1 mol Fe

= 6.0 x 10^-1

There should be only one sig fig. Hoped this helped.

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