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1. Convert the following quantities into moles a. 1000.0 g Mg b. 1000.0 g H₂O c. 1000.0 g NaCl

1. Convert the following quantities into moles a. 1000.0 g Mg b. 1000.0 g H₂O c. 1000.0 g NaCl

Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter8: Chemical Composition
Section: Chapter Questions
Problem 128CP: itamin B12 , cyancobalamin, is essential for human nutrition. Its molecular formula is...
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The molar mass represents not a single atom or molecule but it represents Avogadro's number of atoms or molecules. The formula CS, represents 76.15 g (1 mole) of carbon disulfide. The percentage of sulfur by mass can be calculated as follows: 2S/1 CS₂ = (64.14 g S/76.15 g CS₂) x 100 = 84.22% S The following are examples how the mole concept is applied 1. Mole to gram conversion Determine the number of grams in 4.000 moles of H₂O Molar mass of H₂O = (2 x 1.01) + (1 x 16.00) = 18.02 g/mol 1 mole H₂O = molar mass of H₂O = 18.02 grams H₂O 4.000 mol H₂O x (18.02 g H₂O/ 1 mol H₂O) = 72.08 grams H₂O 2. Gram to mole conversion Determine the number of moles in 88.0 grams of CO₂ Molar mass of CO₂ = (1 x 12.01) + (2 x 16.00) = 44.01 g/mol 1 mole CO₂ = molar mass of CO₂ = 44.01 grams CO₂ 88.0 g CO₂ x (1 mol CO₂ / 44.01 g CO₂) = 2.00 moles CO₂ 3. Mole to molecule conversion Determine the number of molecules of H₂O in 3.00 moles H₂O 1 mole H₂O = 6.022 x 1023 molecules H₂O 3.00 mol H₂O x (6.022 x 1023 molecules H₂O / 1 mol H₂O) = 1.81 x 10²4 molecules H₂O 4. Mole to atoms conversion How many atoms are present in 17.0 moles of water? In order to convert moles of a compound to atoms one must first convert moles into molecules 17.0 mol H₂O x (6.022 x 1023 molecules H₂O/ 1 mol H₂O) = 1.02 x 1025 molecules H₂O The subscripts that appear after the symbol representing an element can be interpreted as atoms of that element in one molecule of the compound 1 molecule H₂O = 2 atoms H + 1 atom O = 3 atoms total Now use this relationship to convert molecules can be converted into atoms 1.02 x 1025 molecules H₂O x (3 atoms / 1 molecule H₂O) = 3.07 x 1025 atoms 174 Units of Chemistry Study Assignment D Scanned with CamScanner
Transcribed Image Text:The molar mass represents not a single atom or molecule but it represents Avogadro's number of atoms or molecules. The formula CS, represents 76.15 g (1 mole) of carbon disulfide. The percentage of sulfur by mass can be calculated as follows: 2S/1 CS₂ = (64.14 g S/76.15 g CS₂) x 100 = 84.22% S The following are examples how the mole concept is applied 1. Mole to gram conversion Determine the number of grams in 4.000 moles of H₂O Molar mass of H₂O = (2 x 1.01) + (1 x 16.00) = 18.02 g/mol 1 mole H₂O = molar mass of H₂O = 18.02 grams H₂O 4.000 mol H₂O x (18.02 g H₂O/ 1 mol H₂O) = 72.08 grams H₂O 2. Gram to mole conversion Determine the number of moles in 88.0 grams of CO₂ Molar mass of CO₂ = (1 x 12.01) + (2 x 16.00) = 44.01 g/mol 1 mole CO₂ = molar mass of CO₂ = 44.01 grams CO₂ 88.0 g CO₂ x (1 mol CO₂ / 44.01 g CO₂) = 2.00 moles CO₂ 3. Mole to molecule conversion Determine the number of molecules of H₂O in 3.00 moles H₂O 1 mole H₂O = 6.022 x 1023 molecules H₂O 3.00 mol H₂O x (6.022 x 1023 molecules H₂O / 1 mol H₂O) = 1.81 x 10²4 molecules H₂O 4. Mole to atoms conversion How many atoms are present in 17.0 moles of water? In order to convert moles of a compound to atoms one must first convert moles into molecules 17.0 mol H₂O x (6.022 x 1023 molecules H₂O/ 1 mol H₂O) = 1.02 x 1025 molecules H₂O The subscripts that appear after the symbol representing an element can be interpreted as atoms of that element in one molecule of the compound 1 molecule H₂O = 2 atoms H + 1 atom O = 3 atoms total Now use this relationship to convert molecules can be converted into atoms 1.02 x 1025 molecules H₂O x (3 atoms / 1 molecule H₂O) = 3.07 x 1025 atoms 174 Units of Chemistry Study Assignment D Scanned with CamScanner
NAME: STUDY ASSIGNMENT D - Chemical Units of Quantity note; Round all molar masses from the Periodic Table to two decimal places 1. Convert the following quantities into moles 1000.0 g Mg a. b. 1000.0 g H₂O c. 1000.0 g NaCl C. d. 1000.0 g H₂ 2. Given 5.400 g of aluminum sulfate How many a. moles of aluminum sulfate are there? b. How many moles of aluminum are there? DATE: How many moles of oxygen are there? Scanned with CamScanner
Transcribed Image Text:NAME: STUDY ASSIGNMENT D - Chemical Units of Quantity note; Round all molar masses from the Periodic Table to two decimal places 1. Convert the following quantities into moles 1000.0 g Mg a. b. 1000.0 g H₂O c. 1000.0 g NaCl C. d. 1000.0 g H₂ 2. Given 5.400 g of aluminum sulfate How many a. moles of aluminum sulfate are there? b. How many moles of aluminum are there? DATE: How many moles of oxygen are there? Scanned with CamScanner
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