der the balanced chemical reaction below. If 24.3 g of iron is produced when 50.0 g (III) oxide and 50.0 g of carbon monoxide react, what is the percentage yield of the on? Fe203(s) + 3 CO(g)→2 Fe(s) + 3 CO2(g)

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Chapter1: Chemical Foundations
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Why is the before (mol) of 2 Fe(s) 0?
der the balanced chemical reaction below. If 24.3 g of iron is produced when 50.0 g
(III) oxide and 50.0 g of carbon monoxide react, what is the percentage yield of the
on?
Fe203(s) + 3 CO(g)→2 Fe(s) + 3 CO2(g)
1
3
NEXT
knowledge of stoichiometry, set up the table below to determine the amounts of each
oduct after the reaction goes to completion (assume 100% yield).
Fe2O3(s)
3 CO(g)
2 Fe(s)
3 CO2(g)
0.313
1.785
-0.313
-0.939
0.626
0.939
0.846
0.626
0.939
RESET
24.3
-24.3
50.0
-50.0
0.435
-0.435
-0.218
0.313
-0.313
1.785
-1.785
0.626
-0.626
Transcribed Image Text:der the balanced chemical reaction below. If 24.3 g of iron is produced when 50.0 g (III) oxide and 50.0 g of carbon monoxide react, what is the percentage yield of the on? Fe203(s) + 3 CO(g)→2 Fe(s) + 3 CO2(g) 1 3 NEXT knowledge of stoichiometry, set up the table below to determine the amounts of each oduct after the reaction goes to completion (assume 100% yield). Fe2O3(s) 3 CO(g) 2 Fe(s) 3 CO2(g) 0.313 1.785 -0.313 -0.939 0.626 0.939 0.846 0.626 0.939 RESET 24.3 -24.3 50.0 -50.0 0.435 -0.435 -0.218 0.313 -0.313 1.785 -1.785 0.626 -0.626
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