You place 3.24 g of iron filings into a test tube with an excess of sulfur, heat the mixture, and then weigh the cooled product.  You get a mass of 4.16 g FeS.  You then use your stoichiometry skills and calculate an expected mass of 5.09 g FeS.   a) Consider each of the values in this problem. Identify the Experimental Yield and Theoretical Yield. Explain your reasoning for each. b) What is the Percent Yield in this scenario? Is this within acceptable range? Please explain. c) Give two potential reasons why the Experimental Yield and Theoretical Yield might not be equal in value.

19. A product weighing 12.11 g was isolated/obtained in the laboratory. The maximum amount of obtainable product was calculated to be 20.51g. What is the percentage (%) yield of this reaction?

Pure magnesium metal is often found as ribbons and can easily burn in the presence of oxygen. When 4.78 g of magnesium ribbon burns with 7.61 g of oxygen, a bright, white light and a white, powdery product are formed. Enter the balanced chemical equation for this reaction. Be sure to include all physical states. equation: What is the limiting reactant? охудen O magnesium The reaction goes to completion, but in the process of recovering the product, some of it was lost. The the percent yield for the reaction is 82.8%. How many grams of product are recovered? mass of product recovered: How many grams of the excess reactant remain? Assume the reaction goes to completion. mass of excess reactant:

Upon reaction of 1.27 gof copper sulfate with excess zinc metal, 0.239 g copper metal was obtained as an experimental result according to the equation: CuSOalaq) + Zn(s) Culs) + ZnSO.laq) Before the experiment was carried out the theoretical yield calculation was completed to predict the maximum amount of copper that could be isolated. The answer was 0.506 g of Cu. What is the percent yield in standard notation?

Please don't provide handwritten solution ....

A chemist recovers 2.76 L of CuSO4(s) in an experiment. What name is given to this volume? a) actual yield.    b) percent yield.    c) standard volume.   d) theoretical yield The theoretical yield for calcium metal in an experiment is 2.78 g. If the percent yield for the experiment was 82.0%, what mass of calcium was obtained? a) 0.0399 g    b) 2.28 g    c) 3.39 g    d) 228 g

The actual yield of one of the reactions in 43.5g. What was theoretical yield in the laboratory if the scientist concluded that % yield of the reaction ended up to be 77%.

What are the steps broken down and calculations to calculate percentage yield, theoretical yield and actual yield in a chemical equation?

A student weighed 0.550 g of lithium chloride, LiCl, to use in a reaction. How many moles is this? Group of answer choices 42.39 5.11 0.0130 23.31 77.08

In a double replacement reaction, 1.214 g of tin(ii) fluoride react with sodium phosphate to form a precipitate. If the tin (ii) phosphate precipitate weighs 1.078 g, what is the percent yield?