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 one year ago
For the following reaction, 4.51 grams of iron are mixed with excess oxygen gas. The reaction yields 5.73 grams of iron(III) oxide.
4 Fe (s) + 3 O2 (g) = 2 Fe2O3 (s)
(1) What is the theoretical yield of iron(III) oxide ?
grams
(2) What is the percent yield for this reaction ?
%
 one year ago
For the following reaction, 4.51 grams of iron are mixed with excess oxygen gas. The reaction yields 5.73 grams of iron(III) oxide. 4 Fe (s) + 3 O2 (g) = 2 Fe2O3 (s) (1) What is the theoretical yield of iron(III) oxide ? grams (2) What is the percent yield for this reaction ? %

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Yahoo!
 one year ago
Best ResponseYou've already chosen the best response.04 Fe (s) + 3 O2 (g) >2 Fe2O3 (s) 56 *4 grams of Fe react with 3 * 32 grams of O2 to give (4*56 + 6*16) of Fe2O3

Yahoo!
 one year ago
Best ResponseYou've already chosen the best response.0So the theoretical yield of iron(III) oxide = 320g = (4*56 + 6*16)

chmvijay
 one year ago
Best ResponseYou've already chosen the best response.0can you tell me what is the molecular weight of CH2Cl2

chmvijay
 one year ago
Best ResponseYou've already chosen the best response.0u only have mentioned the answer what you need

toxicsugar22
 one year ago
Best ResponseYou've already chosen the best response.0For the following reaction, 4.77 grams of iron are mixed with excess oxygen gas. The reaction yields 5.71 grams of iron(III) oxide. 4 Fe (s) + 3 O2 (g) =2 Fe2O3 (s) (1) What is the theoretical yield of iron(III) oxide ? grams (2) What is the percent yield for this reaction ?

toxicsugar22
 one year ago
Best ResponseYou've already chosen the best response.0can you help me on this

toxicsugar22
 one year ago
Best ResponseYou've already chosen the best response.0jsu show me the step

toxicsugar22
 one year ago
Best ResponseYou've already chosen the best response.0how to do this and plus the answer so I get the hang on how to do this
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