SlideServe
Télécharger Obtenir Pro
Menu
Accueil Pro
Préférences
ApparenceLight Aide et commentaires
© SlideServe · v2026

Kwl chart--moles

lea avatar
lea
53 diapositives · 1.1K Views · Aug 10, 2014

Kwl chart--moles. MOLES. This unit test contains 6 types of problems: Molar mass and % composition—must be able to write a chemical formula Grams to moles (using molar mass) Moles to particles/atoms/molecules (using Avogadro’s #)

Kwl chart--moles - slide 1
01 / 53Kwl chart--moles
1 / 17

Télécharger la présentation

Kwl chart--moles
Une image / un lien ci-dessous est fourni (tel quel) pour télécharger la présentation

Politique de téléchargement : le contenu du site vous est fourni TEL QUEL pour votre information et votre usage personnel ; il ne peut être vendu, concédé sous licence ni partagé sur d’autres sites sans l’accord de son auteur.Le contenu vous est fourni TEL QUEL, pour votre information et votre usage personnel uniquement. Téléchargez la présentation en cliquant sur ce lien. Lors du téléchargement, si vous ne parvenez pas à télécharger une présentation, l’éditeur a peut-être supprimé le fichier de son serveur.Pendant le téléchargement, si vous ne parvenez pas à obtenir une présentation, le fichier a peut-être été supprimé par l’éditeur.

F I N

Plus de contenu associé

Transcription de la présentation

  1. Kwl chart--moles

  2. MOLES • This unit test contains 6 types of problems: • Molar mass and % composition—must be able to write a chemical formula • Grams to moles (using molar mass) • Moles to particles/atoms/molecules (using Avogadro’s #) • Grams to moles to particles (using molar mass and Avogadro’s #) • Empirical formulas • Molecular formulas

  3. Mole • The SI (metric) unit used to measure the amount of a substance • 1 mole is always equal to: --Molar mass (g/mole) --Avogadro’s number of particles (6.02 x 1023) --22. 4 Liters of a GAS (AKA molar volume) These may be used as conversion factors when working mole problems.

  4. activator • Define molar mass AND Avogadro’s number.

  5. Molar mass of elements—same as atomic mass • Ex: Titanium 47.867 = 47.9 g/mole (this sample contains Avogadro’s number of atoms) • Ex: oxygen 15.999 = 16.0 g/mole (this sample contains Avogadro’s number of atoms)

  6. Molar Mass of Compounds—must write chemical formula correctly • Multiply the # of atoms for each element by the atomic mass from periodic table Ex:Magnesium hydroxide Mg (OH)2 Mg 1(24.3) = 24.3 O 2(16.0) = 32.0 H 2(1.0) = 2.0 58.3 g/mole (this mass also contains Avogadro’s number of molecules)

  7. Find the molar mass of aluminum sulfate Al 2 (SO4)3 Al 2(27.0) = 54.0 S 3 (32.1)= 96.3 O 12(16.0) = 192.0 342.3 g/mole (this mass also contains Avogadro’s number of molecules)

  8. Calculate the molar mass of diarsenic trioxide.

  9. MOLAR MASS PRACTICE-- • Stannic carbonate • Diarsenicpentasulfide • Hydrofluoric acid

  10. ACTIVATOR: calculate the molar mass • Sucrose

  11. % composition • Shows the % of each element that makes up a compound • Must be calculate molar mass first. Ex: magnesium hydroxide Mg (OH)2 Mg 1 x 24.3 =24.3 24.3/58.3 x 100 = 41.7% O 2 x 16= 32.0 32.0/58.3 x 100 = 54.9% H 2x1.0 = 2.0 58. 3 g/mole 2.0/58.3 x 100 = 3.4%

  12. ACTIVATOR: • Calculate the % composition of sulfurous acid

  13. LAB—BITE THE BUBBLE • SAVE YOUR WRAPPER FOR ENTIRE LAB!! • DO NOT START CHEWING UNTIL YOU SIT DOWN BACK AT YOUR DESK. • CHECK BALANCE TO MAKE SURE IT’S OK BEFORE YOU START!!

  14. READ PROBLEM: • MAKE A HYOTHESIS: • PROCEDURE 1—4 • DATA TABLE 1—5

  15. After chewing: (KEEP YOUR SAME BALANCE) • Procedure 5—8 • Data table 6—8 • Conclusion • Questions 1—2

  16. Calculate the % composition for a sugar substitute called SUCRALOSE

  17. C 12( 12.0) = 144.0 • H 19 (1.0) = 19.0 • Cl 3 (35.5) = 106.5 • O 8 (16.0) = 128.0 397. 5 g/mole % C= 144.0 / 397.5 x 100 = 36.2% % H= 19.0 / 397.5 x 100 = 4.8% % Cl= 106.5 / 397.5 x 100 = 26.8% % O= 128.0/ 397.5 x 100 = 32.2%

  18. Ticket out • 1. Calculate the % composition of carbonic acid. • 2. Calculate the % composition of diantimony trioxide.

  19. 1. H2CO3 H-2 (1.0) = 2.0 3.2% C- 1 (12.0) = 12.0 19.4% O – 3(16.0) = 48.0 77.4% 62.0 g/mole • Sb2O3 Sb- 2(121.8) =243.6 83.5% O – 3(16.0) = 48.0 16.5% 291.6 g/mole

  20. ACTIVATOR • Calculate the molar mass AND % composition of: • C12H22O11 • Cupric sulfate

  21. C: 12 (12.0) = 144.0 • H: 22 (1.0) = 22.0 • O: 11(16.0) = 176.0 CuSO4 Cu: 1(63.5)= 63.5 S: 1 (32.1) = 32.1 O: 4(16.0) = 64.0

  22. Converting Grams to moles Will need to use unit conversion(cancellation) and molar mass will be used for the conversion factor. Ex: 2.50 grams of hydrochloric acid = ____moles H Cl 2.50 grams x 1 mole = 0.0685 moles(3sigfigs) 36.5 grams

  23. Converting moles to grams Ex: 2.50 moles of HCl = __________grams 2.5 moles x 36.5 grams = 91 grams 1 mole (2 sig figs)

  24. Converting particles to moles • Particles, atoms, molecules (synonyms) • Will have to use Avogadro’s number as a conversion factor • Ex: 5.25 x 1025 atoms of Mg = _____moles 5. 25 x 1025 atoms x 1 mole = 87.2 moles 6.02 x 1023 (3 sig figs)

  25. Converting moles to particles 2.50 moles MgO = _________molecules 2.50 moles x 6.02 x 1023 molecules 1 mole = 1.50 x 1024 molecules (3 sig figs)

  26. Converting grams to particles • Will need to use both molar mass AND Avogadro’s number as conversion factors • Will be 2 steps instead of 1 step unit cancellation • Ex: 4.5 grams nitrous acid = __________molecules • HNO2 4.5 g x 1 mole x 6.02 x 1023 molecules = 47 g 1 mole 5.8 x 1022 molecules (2 sig figs)

  27. Converting particles to grams • Ex: 9.35 x 1021 particles of carbon tetrabromide = _____grams C Br4 9.35 x 1021 p x 1 mole x 154 grams = 6.02x1023 p 1 mole 2.39 grams (3 sig figs)

  28. Answers to homework: must show work to receive credit 1. 0.14 mole (gram to moles) 2. 150 g (moles to grams) 3. 1.1 x 1023 molecules (g to molecules) 4 5.30 x 1025 molecules (moles to molecules) 5. 0.074 mole( gram to moles) 6. 0.619 g (particles to grams) 7. 0.49 mole (grams to moles) 8. 0.00083 mole (particles to moles) 

  29. Tab 3 “even more mole problems”—show work to receive credit • 22 g • 1.53 x 1024 molecules • 0.014 g • 7.2 x 1021 molecules • 7.2 x 1023 molecules • 2.08 x 106 g • 56 g • 2.5 g • 31 g • 0.0029 mole • 167 g BONUS: 3.37 x 1026 atoms

  30. activator If grams are converted to moles, use _______________ to convert. If moles are converted to molecules, then use ______________to convert. ****Have calculator, periodic table, and best friend chart****

  31. Mole game All members of your group must show their work on separate sheet of paper. When you calculate the answer, flip the card over to find a word. All of your words will make a sentence. First group to show all work and finish first, wins bonus!

  32. Mole problem diagram Grams-----moles-----particles(atoms or molecules)

  33. Extra practice-mole problems • 55.33 grams of sodium oxide = ____moles • 5.00 x 1022 particles of sodium= _______moles • 2.49 x 1026 atoms of acetic acid = _______________grams

  34. Homework: Video sheet Problems #1—3, 5, 6

  35. ACTIVATOR: Fill in the blanks with multiply/divide OR molar mass/Avogadro’s number: ***When going from moles to grams, _______________ by _____________. ***When going from moles to particles, ____________by _________________. I AM CHECKING 5 HOMEWORK PROBLEMS!!!!

  36. Ticket out Briefly describe the steps for calculating an empirical formula AND molecular formula.

  37. activator Define empirical formula ***both labs due today***

  38. Mole review problems • Convert 5.03 x 1024 molecules of phosphoric acid to grams. • Convert 35.75 grams of dinitrogen monoxide to moles. • Convert 5.0 moles of water to molecules.

  39. answers • 819 grams of H3PO4 • 0.8125 moles of N20 • 3.0 x 1024 molecules of water

  40. Ticket out Tell how to solve for each: • G to moles • Moles to G • Particles to moles • Moles to particles • G to particles • Particles to G

  41. Gum lab—show work to receive credit • HYPOTHESIS, DATA 1—8, CONCLUSION, QUESTIONS 1—4 • 3. MASS OF SUGAR (in grams—data #8)--------MOLES (SUGAR = C12 H22 O11) • 4. MOLES----------PARTICLES

  42. Lab-using the mole • Data Table: mass of empty vial AND substances mass (make sure you’ve subtracted empty vial each time!!) • SHOW WORK TO GET CREDIT • CONVERT GRAMS----------MOLES • CONVERT MOLES---------PARTICLES • ANSWER QUESTIONS 1---5, 6 (BONUS)

  43. Activator: Convert 25.0 moles of water to grams.

  44. activator A molecular formula is a whole number____________of the empirical formula.

  45. EMPIRICAL FORMULAS • Shows the SIMPLEST, WHOLE NUMBER ratio of elements in a compound • Will give you % composition of compound and ask you to find the formulas

  46. Steps for calculating: 1. Change % sign to grams (some problems may already give you grams instead of %) 2. Convert grams to moles (using molar mass) **round to 4 decimals*** 3. Simplify the mole ratio by dividing each one by the smallest 4. Round to the nearest whole number and assign these numbers to the appropriate element

  47. Example: A compound is 78.1% Boron and 21.9% H. Calculate the empirical formula. 78.1 grams B x 1 mole = 7.2315 moles B 10.8 g 21.9 grams H x 1mole =21.9 moles H 1.0 g 7.2315 : 21.9 7.2315 7.2315 1: 3 = BH3

  48. Molecular formulas: Is a WHOLE NUMBER MULTIPLE of the empirical formula You must then first know the empirical formula