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How many milliliters of 0.200 M FeCl3 are needed to react with an excess of Na2S to produce 2.75 g of Fe2S3 if the percent yield for the reaction is 65.0 percent?
Wiki User
∙ 13y ago
.2M x V FeCl3=moles FeCl3 x 1mole Fe2S3/2mole FeCl3=moles of Fe2S3 x mm of Fe2S3/1 mole Fe2S3= g Fe2S3 x .65% yield.
2.75g Fe2S3/ .65= 4.23g Fe2S3/ 207.91= .02035 x 2mole FeCl3=.0407 moles FeCl3/ .2M FeCl3= .2035 L x 1000= 203.5 ml
Wiki User
∙ 13y ago
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Determine the percent yield of a reaction that produces 28.65g of Fe when 50g of Fe2O3 reacts with excess Al according to the following reaction Fe2O3 plus 2Al equals Al2O3 plus 2Fe?
81.93%
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excess,exceed
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A remainder.
What is mean b y hype?
in excess
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92.22%.
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84.62 - 84.66
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94.25 - 94.28
When 300.0 g of ammonia reacted with excess sulfuric acid to produce ammonium sulfate 985.0 g of product were obtained What is the percent yield of ammonium sulfate for this reaction?
84.62 - 84.66 or 84.64%.
Consider a reaction between 5.39 moles of ironIII oxide and excess aluminum in the thermite reaction If 526 g of liquid iron were recovered after the reaction was complete what was the percent yield o?
87.4%
Consider a reaction between 5.39 moles of iron(III) oxide and excess aluminum in the thermite reaction If 526 g of liquid iron were recovered after the reaction was complete, what was the percent yie?
87.4%
Consider a reaction between 8.63 moles of ironIII oxide and excess aluminum in the thermite reaction If 856 g of liquid iron were recovered after the reaction was complete what was the percent yield o?
88.8%
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Because the antacid neutralizes the the HCl in the stomach (or at least in excess amount) to produce water and a salt, and it is good example of neutralization reaction.
Determine the percent yield of a reaction that produces 28.65g of Fe when 50g of Fe2O3 reacts with excess Al according to the following reaction Fe2O3 plus 2Al equals Al2O3 plus 2Fe?
81.93%
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light bulbs technically heat up a filament and if heated to a certain degree it will produce light because of the excess in energy it has
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An acid-base reaction that leaves no excess H+ or OH-
