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Bellwork

Use dimensional analysis to calculate the mass of 2.5 liters of mercury with a density of 13.6 g/ml.

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Bellwork

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  1. Bellwork Solve the following using dimensional analysis and place the answer in scientific notation. 1. Jamie has 2.5 liters of mercury in a jar. What is the mass of this mercury if its density is 13.6 g/ml?

  2. CHAPTER 10THE MOLE

  3. The mole (mol) is one of the seven base units in the SI system. It measures the amount of substance.

  4. The form in which a substance exists is its “representative particle”.Representative particles can be atoms, ions, molecules, formula units, or anything else.

  5. Just as one dozen is 12 representative particles of eggs, a mole is 6.02 x 1023 representative particles. 602,000,000,000,000,000,000,000!!!!!

  6. Examples:1 mole Fe = 6.02 x 1023 atoms of Fe 1 mole H2O molecules = 6.02 x 1023 molecules of water1 mole NaCl formula units = 6.02 x 1023 NaCl formula units1 mole eggs = 6.02 x 1023 eggs You can have a mole of ANYTHING!!

  7. 6.02 X 1023 Watermelon Seeds: Would be found inside a melon slightly larger than the moon. 6.02 X 1023 Donut Holes: Would cover the earth and be 5 miles (8 km) deep. 6.02 X 1023 Pennies: Would make at least 7 stacks that would reach the moon. 6.02 X 1023 Grains of Sand: Would be more than all of the sand on Miami Beach. 6.02 X 1023 Blood Cells: Would be more than the total number of blood cells found in every human on earth. How much is a mole?

  8. Question • How many molecules would be in 3 moles of water?

  9. Diatomic ElementsCertain elements are only stable in pairs or with other elements in a compound. These elements are called the diatomic elements.

  10. There are 7 diatomic elements:Bromine, Iodine, Nitrogen, Chlorine, Hydrogen, Oxygen, and Fluorine(Memory trick: HBrONClIF or 7th Heaven)

  11. Avogadro’s Number*6.02 x 1023 is called Avogadro’s number. *It is named after Amadeo Avogadro who did work in the 1800’s that allowed 6.02 x 1023 to be calculated.

  12. The mole is the “chemist’s dozen”. It is a convenient way to count extremely large numbers of atoms, molecules or ions.

  13. New Conversion Factor!1 mole = 6.02 x 1023 representative particlesWe work these problems using dimensional analysis.

  14. How many moles are 1.20 x 1025 atoms of phosphorous? 1.20 x 1025 atoms P 1 mol P 6.02 x 1023 atoms = 19.9 mol P

  15. How many atoms are in 0.750 mol of Zn? 0.750 mol Zn 6.02 x 1023 atoms Zn = 1 mol Zn 4.52 x 1023 atoms Zn

  16. How many molecules are in 0.400 mol N2O5? 0.400 mol N2O5 6.02 x 1023molecules = 1 mole N2O5 2.41 x 1023 molecules Q: What did Avogadro teach his students in math class? A: Moletiplication

  17. How many moles are contained in 1.20 x 1024 molecules CO2? 1.20 x 1024 molec CO2 1 mol CO2 6.02 x 1023 molecules = 1.99 moles CO2

  18. Question • Your friend gives you a gold ring that contains 2.3 mol of atoms. How many atoms is this?

  19. Gram atomic mass(gam) -atomic mass of an element in grams-mass of one mole of atoms of a monatomic element

  20. Question • Write the atomic masses of the following. • Mg __________ • Cl ___________ • Ba ___________

  21. Example: C =12.0 g = mass of 6.02 x 1023atoms 12.0 g/mol is the gram atomic mass of carbon

  22. Molar mass (M.M.) is a term used to describe the mass of a mole of a chemical compound.

  23. Molar Mass (M.M.)-mass of one mole of any compound-sum of the atomic masses of each atom in the compound 1 mol H2O: 2 mol H 1 mol O =2 mol H x 1.008 g H/mol = 2.016 g =1 mol O x 15.999 g O/mol= 15.999 g 18.015 g H2O

  24. Question • What is the gram molecular mass of P2O5?

  25. What is the molar mass of CH3OH? C 1 x 12.011 = 12.011 H 4 x 1.008 = 4.032 O 1 x 15.999 = 15.999 32.042 g

  26. Quiz day • Get ready for your quiz!!! • Test on Wednesday!

  27. What is the M.M. of magnesium phosphate? Mg3(PO4)2 3 mol Mg 3 x 24.305 g = 72.915 g 2 mol P 2 x 30.974 g = 61.948 g 8 mol O 8 x 15.999 g =127.992 g 262.855 g

  28. What is the molar mass of ammonium sulfate? (NH4)2SO4 2 mol N 2 x 14.007 = 28.014 8 mol H 8 x 1.008 = 8.064 1 mol S 1 x 32.066 = 32.066 4 mol O 4 x 15.999 = 63.996 132.14 g

  29. Mole – Mass ConversionsNew Conversion factor! 1 mol = molar mass ( grams)

  30. Find the mass in grams of 3.32 mol of K. 3.32 mol K 39.098 g K1 mol K = 1.30 x 102 g K

  31. Find the mass in grams of 15.0 mol of sulfuric acid. H2SO4 H 2 x 1.008 = 2.016S 1 x 32.066 = 32.066O 4 x 15.999 = 63.996 98.078 g 15.0 mol H2SO4 98.078 g H2SO4 1 mol H2SO4 = 1470 g H2SO4

  32. Find the number of moles in 11.0 g of methane (CH4). CH4 = (12.011g + 4.032g = 16.043 g) 11.0 g CH4 1 mol CH4 16.043 g CH4 = 0.686 mol CH4 What was Avogadro’s favorite Indian tribe? The MOLEHICANS

  33. Bellwork What is the molar mass of methane? Methane’s formula is CH4

  34. Molti-Step Mole Problems! • Calculate the number of molecules present in 4.29 g of nitrogen dioxide (NO2). • 4.29 g NO2 1 mol NO2 6.02x1023 m.c. NO2= 46.005 g NO2 1 mol NO2 = 5.61x1022 molecules NO2

  35. Molti-Step Mole Problems! • Calculate the number of moles of sulfur atoms present in 2.01 g of sodium sulfide (Na2S). • 2.01 g Na2S 1 mol Na2S 1 mol S atoms 78.046 g Na2S 1 mol Na2S = 0.0258 mol S atoms

  36. Molti-Step Mole Problems! • Calculate the mass in grams of 2.49 x 1020 carbon dioxide (CO2) molecules. 2.49 x 1020 CO2 m.c. 1 mol CO2 44.009 g CO2 6.02x1023 m.c.CO2 1 mol CO2 = 1.82 x 10-2 grams CO2

  37. Molti-Step Mole Problems! • Calculate the grams of carbon in 12.2 mol sucrose, C12H22O11. 12.2 mol C12H22O11 12 mol C atoms 12.011 g C 1 mol C12H22O11 1 mol C atoms = 1.76 x 103 g carbon

  38. Question • Write the two conversion factors we have discussed below. Show how they are related.

  39. Molar Volume of a GasThe volume of a gas is usually measured at 0oC and 1 atmosphere of pressure. This is called standard temperature and pressure (STP).

  40. -At STP, one mole of any gas has a volume of 22.4 L which is called the molar volume of a gas and contains 6.02 x 1023 particles of the gas.-22.4 L of a gas has a mass equal to the gfm of the gas.-So…1 mol = 22.4L = 6.02 x 1023 particles = M.M.

  41. New conversion factor!1 mol of any gas at STP = 22.4 L (for gases only)

  42. What is the volume (liters) at STP of 0.960 mol of methane, CH4? 0.960 mol CH4 22.4 L CH4 1 mol CH4 = 21.5 L CH4

  43. At STP, how many moles are in 0.542 mL of neon gas? 0.542 mL Ne 1 L Ne 1 mol Ne 1000 mL Ne 22.4 L Ne = 2.42 x 10-5 mol Ne

  44. Question • Relate the three conversion factors we have learned below.

  45. Bellwork Jake has a jar full of sodium hydrogen carbonate, or baking soda (NaHCO3). What is the mass of 2.78 mol baking soda?

  46. Bellwork How many propane molecules are in 25.00 g of propane, C3H8?

  47. Percent Composition(remember: percent = part divided by total x 100)percent by mass of each element in a compound

  48. What is the percent composition of NO2? NO2 N 1 x 14.007 = 14.007 O 2 x 15.999= 31.998 ( /46.005g)x100 =30.4%Ca ( /46.005g)x100 =69.6% C 46.005 100% As long as your % adds up to 99-101% you are fine.

  49. Why is Avogadro so rich! Because he is a multi-mole-ionairre!!!!

  50. What is the percent composition of calcium acetate? Ca(C2H3O2)2 Ca1 x40.078=40.078 C 4 x12.011=48.044 H 6 x 1.008= 6.048 O 4 x15.999=63.996 158.166 g ( /158.166g)x100=25.3% Ca ( /158.166g)x100=30.4% C ( /158.166g)x100=3.8% H ( /158.166g)x100=40.5% O 100.0%

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