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Mass of crucible + lid 18.30 08 Y 18.8979g 18.62009 |8.८1१। १ From the data above, calculate the mass of the anhydrous compound (= the residue) and the mass of water lost by Mass of crucible and hydrate + lid 3 Mass of crucible and residue + lid (1st heating) Mass of crucible and residue + lid (2nd heating)" Mass of crucible and residue + lid (3rd heating)" Mass of lid (just in case!) 8.47619 "USE THE LAST HEATING PERFORMED FOR ALL CALCULATIONS. CALCULATIONS: SHOW YOUR WORK – WORK ALONE 1. If we use good technique (avoid spills, etc.) then the following will be true. mass of hydrate = mass of the residue + mass of the water lost subtracting the appropriate masses. Copy the descriptions for the lines you are using from the tabio. Mass ofMa ss af Crubile and hydicte Mass of Mass of Ciucible tlid tid 18.8979% - 18.3008g 0.5971 Mass of hydrate (starting material) %3D Mass of MasS Ciralble and residee 18 o6191 Mass of Mass of Crucible trido 18.3008 0.3183 Mass of anhydrous compound (residue) Mass of Mass Crucible a nd Mass ofMa Ss uf Crucible and residueNd 18.8979 18.6191. 0.2788 Mass of water lost %3D 2. Determine the percent salt (M9SO4, by mass) in the hydrate (starting compound): 3. Use the data and calculations above to determine the percent water (by mass) in the hydrate (starting compound). If a different sample of your unknown contained 1.343 g of water, how many grams of MgSO4 would it contain? Use dimensional analysis and the mass percentage calculations from #2 and #3: 4.

Mass of crucible + lid 18.30 08 Y 18.8979g 18.62009 |8.८1१। १ From the data above, calculate the mass of the anhydrous compound (= the residue) and the mass of water lost by Mass of crucible and hydrate + lid 3 Mass of crucible and residue + lid (1st heating) Mass of crucible and residue + lid (2nd heating)" Mass of crucible and residue + lid (3rd heating)" Mass of lid (just in case!) 8.47619 "USE THE LAST HEATING PERFORMED FOR ALL CALCULATIONS. CALCULATIONS: SHOW YOUR WORK – WORK ALONE 1. If we use good technique (avoid spills, etc.) then the following will be true. mass of hydrate = mass of the residue + mass of the water lost subtracting the appropriate masses. Copy the descriptions for the lines you are using from the tabio. Mass ofMa ss af Crubile and hydicte Mass of Mass of Ciucible tlid tid 18.8979% - 18.3008g 0.5971 Mass of hydrate (starting material) %3D Mass of MasS Ciralble and residee 18 o6191 Mass of Mass of Crucible trido 18.3008 0.3183 Mass of anhydrous compound (residue) Mass of Mass Crucible a nd Mass ofMa Ss uf Crucible and residueNd 18.8979 18.6191. 0.2788 Mass of water lost %3D 2. Determine the percent salt (M9SO4, by mass) in the hydrate (starting compound): 3. Use the data and calculations above to determine the percent water (by mass) in the hydrate (starting compound). If a different sample of your unknown contained 1.343 g of water, how many grams of MgSO4 would it contain? Use dimensional analysis and the mass percentage calculations from #2 and #3: 4.

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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Use the calculated masses of the anhydrous compound and water (from #1) and the identity of the hydrated compound (on the provided data slip) to determine the formula of the hydrated compound. 5. Mass of anhydrous compound (from #1): Mass of water lost (from #1): A. Calculate moles of the anhydrous compound (MgSO.): B. Calculate moles of water: C. Determine the simplest mole ratio to find the empirical formula: (Note: unlike with determining formulas for compounds, you may round to the nearest whole number for the moles of water in the hydrate) Formula of the hydrate: M9SO4• _H2O 6. Hydrate #2: Data for hydrate #2 (supplied on the data slip) Slip # Mass of hydrate before heating Mass of residue after heating (= anhydrous compound) Loss of mass upon heating (= water) A. Calculate moles of the anhydrous compound (M9SOA): B. Calculate moles of water: C. Determine the simplest mole ratio to find the empirical formula: Formula of the hydrate: MgSO4:- _H2O
Transcribed Image Text:Use the calculated masses of the anhydrous compound and water (from #1) and the identity of the hydrated compound (on the provided data slip) to determine the formula of the hydrated compound. 5. Mass of anhydrous compound (from #1): Mass of water lost (from #1): A. Calculate moles of the anhydrous compound (MgSO.): B. Calculate moles of water: C. Determine the simplest mole ratio to find the empirical formula: (Note: unlike with determining formulas for compounds, you may round to the nearest whole number for the moles of water in the hydrate) Formula of the hydrate: M9SO4• _H2O 6. Hydrate #2: Data for hydrate #2 (supplied on the data slip) Slip # Mass of hydrate before heating Mass of residue after heating (= anhydrous compound) Loss of mass upon heating (= water) A. Calculate moles of the anhydrous compound (M9SOA): B. Calculate moles of water: C. Determine the simplest mole ratio to find the empirical formula: Formula of the hydrate: MgSO4:- _H2O
From the data above, calculate the mass of the anhydrous compound (= the residue) and the mass of water lost by subtracting the appropriate masses. Copy the descriptions for the lines you are using from the table. 1 Mass of crucible + lid 18.30 08 Y 18.8979g 18.62009 18.6191 Mass of crucible and hydrate + lid 3 Mass of crucible and residue + lid (1st heating) 4 Mass of crucible and residue + lid (2nd heating)" Mass of crucible and residue + lid (3rd heating)" Mass of lid (just in case!) 8.47619 *USE THE LAST HEATING PERFORMED FOR ALL CALCULATIONS. CALCULATIONS: SHOW YOUR WORK – WORK ALONE 1. If we use good technique (avoid spills, etc.) then the following will be true: mass of hydrate = mass of the residue + mass of the water lost Smel Mass of Ma ss f Crubile and hydicte Mass of Mass of Cincible tlid tid 18.8979% 18.30088 0.5971 Mass of hydrate (starting material) %3D Mass of Cvalble and res,ide o6191 Mass of Flid Mass of Mass of Crucible tilid 18.3008 0.3183 Mass of anhydrous compound (residue) %3D Mass of Mass crucible a nid फनुननडो Q Crucib le and 18.8979 18.6191 0.2788 Mass of Ma SS residue Mass of water lost %3D 2. Determine the percent salt (MgSO4, by mass) in the hydrate (starting compound): 3. Use the data and calculations above to determine the percent water (by mass) in the hydrate (starting compound). 4. If a different sample of your unknown contained 1.343 g of water, how many grams of M9SO4 would it contain? Use dimensional analysis and the mass percentage calculations from #2 and #3:
Transcribed Image Text:From the data above, calculate the mass of the anhydrous compound (= the residue) and the mass of water lost by subtracting the appropriate masses. Copy the descriptions for the lines you are using from the table. 1 Mass of crucible + lid 18.30 08 Y 18.8979g 18.62009 18.6191 Mass of crucible and hydrate + lid 3 Mass of crucible and residue + lid (1st heating) 4 Mass of crucible and residue + lid (2nd heating)" Mass of crucible and residue + lid (3rd heating)" Mass of lid (just in case!) 8.47619 *USE THE LAST HEATING PERFORMED FOR ALL CALCULATIONS. CALCULATIONS: SHOW YOUR WORK – WORK ALONE 1. If we use good technique (avoid spills, etc.) then the following will be true: mass of hydrate = mass of the residue + mass of the water lost Smel Mass of Ma ss f Crubile and hydicte Mass of Mass of Cincible tlid tid 18.8979% 18.30088 0.5971 Mass of hydrate (starting material) %3D Mass of Cvalble and res,ide o6191 Mass of Flid Mass of Mass of Crucible tilid 18.3008 0.3183 Mass of anhydrous compound (residue) %3D Mass of Mass crucible a nid फनुननडो Q Crucib le and 18.8979 18.6191 0.2788 Mass of Ma SS residue Mass of water lost %3D 2. Determine the percent salt (MgSO4, by mass) in the hydrate (starting compound): 3. Use the data and calculations above to determine the percent water (by mass) in the hydrate (starting compound). 4. If a different sample of your unknown contained 1.343 g of water, how many grams of M9SO4 would it contain? Use dimensional analysis and the mass percentage calculations from #2 and #3:
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