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CHEMISTRY Unit 3 Plan – Moles Name ______________________ Assignments A) Mole notes /ws (pg 3-4 in packet) B) More mole practice ws (pg 5-6 in packet) C) Mole lab D) Expt #8 – iron and copper chloride E) More TBA Text Support Study pg 45-46 (intro to the mole) Study pg 53-55 (molar mass and mole conversions) Study pg 250-253 (focus on percent composition on pg 251) On-Line Text: www.lab-aids.com Username: evhs1 Password: smeyer (Log in as student in upper right corner. This is a common username and password for all my chemistry students.) Learning Targets (I can …) A) Differentiate between atoms, molecules, and formula units. B) State Avogadro’s hypothesis and discuss its importance in the development of the mole concept. C) State the definitions of a mole. D) Determine the molar mass of elements and compounds. E) Perform problem solving conversions for moles, grams, atoms, and molecules (operating the mole train). F) Perform chemical reactions, collect data on them, and mathematically determine the mole relationships involved. G) Find the % composition (by mass) of compounds and other substances. H) Discuss examples of chemistry outside the classroom. UNITS AND TERMS TO KNOW AND MEMORIZE A) Avogadro’s hypothesis – Equal volumes of gases, measured at the same temperature and pressure contain equal number of particles. B) One mole = 6.0 x 1023 One mole of any gas at STP (standard temperature and pressure) has a volume of 22.4 liters. STP means temperature = 0ºC and pressure = 760 mm Hg or 1.00 atmosphere. Tentative Schedule Mon 10/1 The mole, molar mass, and the mole train Tue 10/2 Qand A Wed 10/3 Mole Lab Thu 10/4 Quiz; Expt #8 --- Lab Day #1 Fri 10/5 Expt #8 --- Lab Day #2 Mon Tue Wed 10/8 Expt #8 --- Lab Day #3 10/9 Review / practice exam 10/10 Exam #3 Unit #3 packet due On-line support Mr. Guch’s website http://misterguch.brinkster.net/explains2.html (check out “finding molar masses” and “mole calculations” sections for excellent coverage of unit 3 topics) This website will help you out in your quest to understand chemistry. Explanations are at the introductory level and give some detail --- but not too much. Even the humor is above average. You need to check this out. ChemTeam www.chemteam.info (see section on “the mole”) This website may help you in your quest to understand chemistry. Explanations can get quite involved – depending on the topic. It may be helpful at the introductory level. It will be especially helpful if you are looking for extra detail. Chem – Some Unit 3 HW Answers Scientific Notation Review (pg 3) 1. 3.5 x 10-3 2. 6.09 x 1010 3. 5.6789 x 104 1. 123,000 2. 0.00035 3. 9990 Molar Mass (pg 3) Answers in sequence for #1-4 1. 17.0 g/mol 2. 100.1 g/mol Mole Practice (pg 3-4) Answers in sequence for #1-15 1. 2.4 x 1024 atoms 5. 5.0062 mol 9. 16.0 g/mol 13. 2.1999 mol 2. 2.51 mol 3. 294 g 4. 4900 g 6. 3.4997 mol 7. 2.1076 x 1024 atoms 8. 176 g 10. 96 g 11. 62.0 g/mol 12. 0.8 mol 14. 1.3238 x 1024 molecules 15. 6.7 x 1023 molecules More Mole Problems (pg 5-6) Answers scrambled within each number. #1 236 g 1.8 x 10-6 g #2 2.6 x 1024 atoms 4.6 x 1021 atoms 22 23 #3 1 x 10 1.3 x 10 3.48 x 1021 -5 #4 2 x 10 mol 0.0578 mol #5 114 g #6 1.8 x 1020 molecules 3.3 x 1025 molecules #7 35 g 3.6 x 1023 molecules #8 7.8% and 92.2% 42.1%, 6.4% and 51.5% 92.3% and 7.7% 8.1%, 53.7% and 38.3% 3. 44.0 g/mol 4. 182.7 g/mol 27.3 g 460 g 13.6 g 24 2.6 x 10 atoms 2.6 x 1024 (all in molecules) 1320 mol 3.939 mol 3.0 x 10-4 mol Name Hour Mole Notes A mole is just a number used commonly in chemistry. There are 6.022 x 1023 particles in a mole. (Avagadro’s Number) Each element has different sized atoms. Because of the different sizes, each element has a different mass for 6.022 x 1023 (1 mole) of atoms. The molar mass (mass of 1 mole) of an element is equal to the atomic mass on the periodic table. Helium molar mass = 4.003 g/mol You can find the molar mass of a compound by adding all the masses of each element in the compound. o Example: H2O: 2 H (1.0 g/mol) + 1 O (16.0 g/mol) = 18.0 g/mol of water Scientific Notation Review: Write the following numbers in scientific notation: 1. 0.0035 _________________________ 2. 60900000000 _________________________ 3. 56789 _________________________ Write out the following numbers: 1. 1.23 x 105 _________________________ 2. 3.5 x 10-4 _________________________ 3. 9.99 x 103 _________________________ Molar Mass – Calculate the molar mass of the following compounds. 1. NH3 2. CaCO3 3. CO2 4. Ni(NO3)2 Mole Practice 1. How many atoms are present in 4 moles of any element? 2. How many moles are there in 1.51 x 1024 atoms? 3. Determine the mass in grams of 4.5 moles of zinc. 4. Determine the mass in grams of 25 moles of gold. 5. Determine the number of moles in 160.35 g of sulfur. 6. Determine the number of moles of 415.45 g of tin. 7. Determine the number of atoms in the amount of tin from #6. 8. What would be the mass of 4 moles of CO2? 9. What is the molar mass of methane, CH4? 10. What would be the mass of 6 moles of CH4? 11. What is the molar mass of carbonic acid, H2CO3? 12. How many moles of carbonic acid are in 50 grams? 13. How many moles are in 128.57 grams of NaCl? 14. How many molecules (formula units) are in the amount of NaCl from #13? 15. How many molecules (formula units) are in 150 g of CuCl2? More Mole Problems (Unit #3 Practice) Name ______________________ All Aboard! Here’s an opportunity to ride the mole train. Show all work and use appropriate units. You may need additional paper. This worksheet will function as both an opportunity to solve mole train problems and a review sheet for unit #3. Practice. Ask questions. Good luck! 1. Calculate the following in grams … a. 0.43 moles of Cu b. 1.13 moles of C c. 2.41 moles of H2SO4 d. 1.2 x 1025 atoms of Na e. 6.4 x 1015 molecules of AgNO3 2. Calculate the following in atoms … a. 4.3 moles of Au b. 4.3 moles of He c. 0.31 grams of Ca 3. Calculate the following in molecules … a. 4.3 moles of NaCl b. 0.02 moles of H2O c. 21 grams of CaCO3 d. 1.12 grams of K2CrO4 4. Find the amount of moles in … a. 3.48 x 1022 molecules of CuBr2 b. 231.2 grams of Ni c. 0.004 grams of AgNO3 d. 7.96 x 1026 atoms of Pb 5. One liter of Kool-Aid contains 2.0 x 1023 molecules of sugar (C12H22O11). What mass of sugar is present in this sample? 6. A 1000 mL sample of lake water contains 0.0095 grams of dissolved oxygen molecules (O2). This corresponds to a dissolved oxygen reading of 9.5 ppm. a. How many moles of dissolved oxygen molecules (O2) are present? b. How many molecules of dissolved oxygen (O2) are present? c. How many molecules of water (H2O) are present?(Hint: For water 1000 mL = 1000 g) 7. One liter of ocean water contains 0.60 moles of NaCl. a. What mass of NaCl is this? b. How many molecules of NaCl is this? 8. Find the percent composition (by mass) of each element in the following molecules … a. C6H6 b. CCl4 c. C12H22O11 d. CBrF3