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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 129.4 g ZnS, 1 mole ZnS, 1 mole Zn 8.47 g Zn × = 16.8 g ZnS, 65.4 g Zn 1 mole S 1 mole ZnS, 129.4 g ZnS, 1 mole ZnS, 6.03 g S x = 12.2 g ZnS, 32.0 g S 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 decima place.

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 129.4 g ZnS, 1 mole ZnS, 1 mole Zn 8.47 g Zn × = 16.8 g ZnS, 65.4 g Zn 1 mole S 1 mole ZnS, 129.4 g ZnS, 1 mole ZnS, 6.03 g S x = 12.2 g ZnS, 32.0 g S 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 decima 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 Zn 1 mole ZnS, 1 mole Zn 129.4 g ZnS, 1 mole ZnS, 8.47 g Zn × = 16.8 g ZnS, %3D 65.4 g Zn 1 mole ZnS, 129.4 g ZnS, 1 mole ZnS, 1 mole S 6.03 g S × = 12.2 g ZnS, 32.0 g S 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 Zn 1 mole ZnS, 1 mole Zn 129.4 g ZnS, 1 mole ZnS, 8.47 g Zn × = 16.8 g ZnS, %3D 65.4 g Zn 1 mole ZnS, 129.4 g ZnS, 1 mole ZnS, 1 mole S 6.03 g S × = 12.2 g ZnS, 32.0 g S 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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