Combining 0.300 mol Fe2O30.300 mol Fe2O3 with excess carbon produced 12.8 g Fe.12.8 g Fe. Fe2O3+3C⟶2Fe+3COFe2O3+3C⟶2Fe+3CO What is the actual yield of iron in moles? actual yield:________mol What is the theoretical yield of iron in moles? theoretical yield:_______mol What is the percent yield?

Combining 0.300 mol Fe2O30.300 mol Fe2O3 with excess carbon produced 12.8 g Fe.12.8 g Fe. Fe2O3+3C⟶2Fe+3COFe2O3+3C⟶2Fe+3CO What is the actual yield of iron in moles? actual yield:__mol What is the theoretical yield of iron in moles? theoretical yield:_mol What is the percent yield?

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter4: Stoichiometry Of Chemical Reactions

Section: Chapter Questions

Problem 65E: Freon-12, CCl2F2, is prepared from CCl4 by reaction with HF. The other product of this reaction is...

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Concept explainers

Mole Concept

Mole concept is a method to determine the amount of any substance that consists of some elemental particles using a grouping unit called ‘mole’. The mole concept enables one to handle the large amount of small elementary particles. The mole concept can be used in many calculations related to mole calculation, molar amount, mole ratio, and so on, which are significant in chemistry.

Question

Combining 0.300 mol Fe2O30.300 mol Fe2O3 with excess carbon produced 12.8 g Fe.12.8 g Fe.

Fe2O3+3C⟶2Fe+3COFe2O3+3C⟶2Fe+3CO

What is the actual yield of iron in moles?

actual yield:________mol

What is the theoretical yield of iron in moles?

theoretical yield:_______mol

What is the percent yield?

percent yield:________%

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A chemistry student performed the reaction: SnCl4(l) + 2H2Se(g) -> SnSe2(s) + 4HCl(g) in lab. The student started with 0.34 moles of SnCl4 and 0.46 moles of H2Se. The amount of HCl(g) actually produced by the student was 0.26 moles of HCl. a. what is the limiting reagent? b. what is the % yield for this reaction?
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