Using number 1's information what would be my amount of moles of water? Also, did I do number 4 and 5 correctly? Chemical FormulaPrelab QuestionsName: Ashlyn NewtonSection:_OoPrepare For It! Pre-Lab Questions1. If 1.07 g of CUx(SO4)y z H2O(s) is heated to form 0.80 g of the dehydrated Cux(SO4)y(s), determine thegrams (and moles) of water lost:water lost|= U.015 moles water lost2. If the dehydrated compound was found to contăain 0.31 g Cu, determine the moles of Cu:morecular mass Cu= 63-59/mol18318= 0.0049 moles(63.5glm3. Determine the grams of sulfate by difference (g Cux(SO4)y - g Cu), and then convert to moles sulfate (useMM of SO4)mass cusau)y=0-8 mass Cu=0.319mass So4=(0.8-0-31=0.49gmoles of sulfate - 0.499a s galmoここのmolęcular mass4. Determine the mole ratios by dividing by the smallest moles:moles copper0190.005= Xsmallest molesmoles sulfate|=てO」こIIsmallest molesmoles water= Zsmallest molesこ5. Write the formula:6. Name the hydrate:Determination of a Chemical FormulaPage 9 of 9

4.) Mole ration is calculated by dividing the least value of moles by each value. 5.) We use mole…

Chemical Formula Prelab Questions Name: Ashlyn Neurton Section: O0 Prepare For It! Pre-Lab Questions 1. If 1.07 g of Cux(SO4)y z H20(s) is heated to form 0.80 g of the dehydrated Cux(SO4)v(s), determine the grams (and moles) of water lost: (1.07-08)9 - 0.279 water lost 0.27 = O. 015 moles water lost 2. If the dehydrated compound was found to contain 0.31 g Cu, determine the moles of Cu: molecular mass Cu=63-Sa/ mol 18. ダの (63. Sglm = 0.0049 moles 3. Determine the grams of sulfate by difference (g Cux(SO4)y - g Cu), and then convert to moles sulfate (use MM of SO4) mass cusau)y = 0.8 mass Cu=0.319 moles of sulfate-0.492 *0.005 mol wCのね %3D b60=て18:0-8.0)-hos ssmu 4. Determine the mole ratios by dividing by the smallest moles: molecular maşs Aelmo| moles copper = X smallest moles moles sulfate 0.005 |=て」こ smallest moles moles water = Z smallest moles 0.015 とこ0E-とheo 5. Write the formula: 6. Name the hydrate:

Chemical Formula Prelab Questions Name: Ashlyn Neurton Section: O0 Prepare For It! Pre-Lab Questions 1. If 1.07 g of Cux(SO4)y z H20(s) is heated to form 0.80 g of the dehydrated Cux(SO4)v(s), determine the grams (and moles) of water lost: (1.07-08)9 - 0.279 water lost 0.27 = O. 015 moles water lost 2. If the dehydrated compound was found to contain 0.31 g Cu, determine the moles of Cu: molecular mass Cu=63-Sa/ mol 18. ダの (63. Sglm = 0.0049 moles 3. Determine the grams of sulfate by difference (g Cux(SO4)y - g Cu), and then convert to moles sulfate (use MM of SO4) mass cusau)y = 0.8 mass Cu=0.319 moles of sulfate-0.492 *0.005 mol wCのね %3D b60=て18:0-8.0)-hos ssmu 4. Determine the mole ratios by dividing by the smallest moles: molecular maşs Aelmo| moles copper = X smallest moles moles sulfate 0.005 |=て」こ smallest moles moles water = Z smallest moles 0.015 とこ0E-とheo 5. Write the formula: 6. Name the hydrate:

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter9: Chemical Quantities

Section: Chapter Questions

Problem 36QAP

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