Help understanding step 3. Can someone explain why I can't use Alternative step 3 instead of 3 since we have mass of ZnS produced. And why step 3 uses Zn's exten of reaction? Question: Calculate the theoretical yield of zinc sulphide, in grams, from the reaction of 0.5g zinc and 0.5g sulphur. If the actual yield is 0.6gZnS, what is the percentage yield? 8Zn+S →8ZnS = extent of 0.5(g) = 1.95 x 10 mol Step 3: Z Sn= Exv=9.56 x 10 molx c = 7.65 x 10 mol Alternative step 256.48_olx 1 m Mxv step 1: Z₁ = 0.5(g) 65.38_olx8 =9.56 x 10 mol Step 2: S= m m - raction= = v 3Z = 0.68 97.474 ol m

Help understanding step 3. Can someone explain why I can't use Alternative step 3 instead of 3 since we have mass of ZnS produced. And why step 3 uses Zn's exten of reaction? Question: Calculate the theoretical yield of zinc sulphide, in grams, from the reaction of 0.5g zinc and 0.5g sulphur. If the actual yield is 0.6gZnS, what is the percentage yield? 8Zn+S →8ZnS = extent of 0.5(g) = 1.95 x 10 mol Step 3: Z Sn= Exv=9.56 x 10 molx c = 7.65 x 10 mol Alternative step 256.48_olx 1 m Mxv step 1: Z₁ = 0.5(g) 65.38_olx8 =9.56 x 10 mol Step 2: S= m m - raction= = v 3Z = 0.68 97.474 ol m

Living By Chemistry: First Edition Textbook

1st Edition

ISBN:9781559539418

Author:Angelica Stacy

Publisher:Angelica Stacy

ChapterU4: Toxins: Stoichiometry, Solution Chemistry, And Acids And Bases

Section: Chapter Questions

Problem 12RE

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