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A chemist goes into the lab and performs an experiment in which a mixture of 8.47 grams of Zn and 6.03 g of sulfur are reacted. Before starting the experiment they perform the following calculations to predict the maximum (theoretical) yield of zinc sulfide that could be produced. First, write a balanced equation: Zn + 2 S ZnS2 Second, check to see which reagent is limiting: 1 mole Zn 65.4 g Zn 1 mole ZnS, 1 mole Zn 129.4 g ZnS, 1 mole ZnS, 8.47 g Zn x = 16.8 g ZnS, 1 mole ZnS, 1 mole S 32.0 g S 129.4 g ZnS, 1 mole ZnS, 6.03 g Sx = 12.2 g ZnS, 2 moles S Since 6.03 g S produces the least amount of ZnS2, the S is limiting! They obtain an actual yield of 8.25 grams of zinc sulfide. Calculate their percent yield to one decimal place.

A chemist goes into the lab and performs an experiment in which a mixture of 8.47 grams of Zn and 6.03 g of sulfur are reacted. Before starting the experiment they perform the following calculations to predict the maximum (theoretical) yield of zinc sulfide that could be produced. First, write a balanced equation: Zn + 2 S ZnS2 Second, check to see which reagent is limiting: 1 mole Zn 65.4 g Zn 1 mole ZnS, 1 mole Zn 129.4 g ZnS, 1 mole ZnS, 8.47 g Zn x = 16.8 g ZnS, 1 mole ZnS, 1 mole S 32.0 g S 129.4 g ZnS, 1 mole ZnS, 6.03 g Sx = 12.2 g ZnS, 2 moles S Since 6.03 g S produces the least amount of ZnS2, the S is limiting! They obtain an actual yield of 8.25 grams of zinc sulfide. Calculate their percent yield to one decimal place.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A chemist goes into the lab and performs an experiment in which a mixture of 8.47 grams of Zn and 6.03 g of sulfur are reacted. Before starting the experiment they perform the following calculations to predict the maximum (theoretical) yield of zinc sulfide that could be produced. First, write a balanced equation: Zn + 2 S ZnS2 Second, check to see which reagent is limiting: 1 mole ZnS, 1 mole Zn 65.4 g Zn 129.4 g ZnS, 1 mole ZnS, 8.47 g Zn x = 16.8 g ZnS,2 1 mole Zn 129.4 g ZnS, 1 mole ZnS, 1 mole ZnS, 1 mole S 32.0 g S 12.2 g ZnS, 6.03 g Sx 2 moles S Since 6.03 g S produces the least amount of ZnS2, the S is limiting! They obtain an actual yield of 8.25 grams of zinc sulfide. Calculate their percent yield to one decimal place.
Transcribed Image Text:A chemist goes into the lab and performs an experiment in which a mixture of 8.47 grams of Zn and 6.03 g of sulfur are reacted. Before starting the experiment they perform the following calculations to predict the maximum (theoretical) yield of zinc sulfide that could be produced. First, write a balanced equation: Zn + 2 S ZnS2 Second, check to see which reagent is limiting: 1 mole ZnS, 1 mole Zn 65.4 g Zn 129.4 g ZnS, 1 mole ZnS, 8.47 g Zn x = 16.8 g ZnS,2 1 mole Zn 129.4 g ZnS, 1 mole ZnS, 1 mole ZnS, 1 mole S 32.0 g S 12.2 g ZnS, 6.03 g Sx 2 moles S Since 6.03 g S produces the least amount of ZnS2, the S is limiting! They obtain an actual yield of 8.25 grams of zinc sulfide. Calculate their percent yield to one decimal place.
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