Fe2O3 (s) + CO (g) ----> Fe (s) + CO2 13.5 g of Fe2O3 is reacted...
Fe2O3 (s) + CO (g) ----> Fe (s) + CO2
13.5 g of Fe2O3 is reacted with 15.0 g of Co. 8.30 g of Fe is obtained. Identify the limiting reagent and calculate the theoretical yield and percent yield for Fe.
Homework Answers
Balanced reaction :
Fe2O3 + 3CO -> 2Fe + 3CO2
According to the reaction,
1 mole Fe2O3 require 3 mole CO
159.69 g Fe2O3 require 3×28 = 84 g CO
13.5 g Fe2O3 require 84×13.5/159.69 g CO
= 7.10 g CO
Since we have more CO available hence Fe2O3 is limiting reagent.
According to the reaction,
159.69 g Fe2O3 give 2 mole Fe
159.69 g Fe2O3 give 2×55.8 = 111.69 g Fe
13.5 g Fe2O3 give 111.69×13.5/159.69 g Fe
= 9.44 g Fe
Hence, theoretical yield = 9.44 g
Percent yield = 8.30×100/9.44
= 87.92%
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Taking Pool 3 Time Remaining:02:43:54 1. CO(g) and Fe2O3(s) react to form Fe(s) and CO2(g). What is the theoretical yield of Fe(s) if the percent yield of Fe(s) is 61.0% and 84.0 grams of Fe(s) forms. 138. grams 221. grams 51.2 grams 110. grams 193. grams Use the slider to rate your confidence on this question. 100 Not at all confident Very confident
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Fe(s) + CO2(g)
Given: Fe2O3(S) + CO(g)
2FeO(s) + CO2(g) H=
+38 kJ
Fe2O3(s) + 3CO(g)
2Fe(s) + 3CO2(g)
H=
-28 kJ
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Given the following reactions:
Fe2O3(s) + 3 CO(g)2
Fe(s)+ 3 CO2(g)
H=-28.0kJ
2 Fe(s) + 4 CO2(g)4
CO(g) + Fe3O4(s)
H = +12.5 kJ
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H
for this reaction: FeO(s) + CO(g)
Fe(s) + CO2(g)
Given: Fe2O3(S) + CO(g)
2FeO(s) + CO2(g) H=
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2Fe(s) + 3CO2(g)
H=
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Fe2O3(s) + 3 CO(g)2
Fe(s)+ 3 CO2(g)
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