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Ch10.1 – The Mole

Ch10.1 – The Mole. 1 mol = 6.02 x 10 23 particles This is called Avogadro’s Number *Think of it as a chemist’s dozen (A dozen donuts or a mole of donuts?) Can be used for atoms, ions, molecules, donuts, oranges, grains of sand, chevys , etc. Why that number?

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Ch10.1 – The Mole

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  1. Ch10.1 – The Mole 1 mol = 6.02 x 1023 particles This is called Avogadro’s Number *Think of it as a chemist’s dozen (A dozen donuts or a mole of donuts?) Can be used for atoms, ions, molecules, donuts, oranges, grains of sand, chevys, etc. Why that number? -Since 1 amu = 1.66 x 10-24g: .000 000 000 000 000 000 000 00166 x 602 000 000 000 000 000 000 000 = 1

  2. The Mole • Can use as a unit for counting numbers • Atoms are too small to count individually and there are too many, so we need a way to bundle a bunch, like having a dozen oranges = 12 oranges • 1 mole = 6.02 x 1023 particles • This is hard to understand, so let’s relate it. Did You Know??? A grain of rice has an average mass of 1.75 x 10-5kg.What is the mass of one mole, 6.02 x 1023, grains of rice? 1.05 x 1019 kilogramsThis is hard to understand, so let’s change this mass to the mass of cars.This would require a million cars per person to equal this mass!! You can count the number of oranges in 6 dozen in a few minutes.Six moles of oranges would have a mass as large as the entire Earth! Avogadro’s number (1 mole) is so large, if you could count 100 particles everyminute and counted 12 hrs every day, and had every person on Earth alsocounting, it would take more than 4 million years to count a mole of anything! To obtain Avogadro’s number in grains of sand, it would be necessary to dig upthe entire surface of the Sahara Desert, an area of 8 x 106km2 (an area slightlyless than the area of the U.S.), to a depth of 200m.

  3. Ex 1) How many moles of Mg are 3.01 x 1022 atoms? Ex 2) How many molecules are 4.00 mol of glucose, C6H12O6? HW #2) How many atoms are 0.360mol of Silver? Conversions: 1 mol 6.02 x 1023 particles or 1 mol 6.02 x 1023 particles

  4. Gram Formula Mass Ex3) He weighs or C weighs or The mole # was chosen so that the # on the Periodic Table can be read in grams. *Round masses to nearest 1/10* Ex4)H 1.0079 F 18.998403 Cl 35.453

  5. Ex5) Find the molecular mass of: H2O NaCl Mg3 (PO4)2 Ch 10 HW #1 1 – 7

  6. Ch10 HW#1 1 – 7 1) How many moles in 2.80 x 1024 atoms of silicon? 3) How many oxygen atoms in each:A) NH4NO3B) C9H8O4C) O3D) C3H5(NO3)3

  7. Ch10 HW#1 1 – 7 1) How many moles in 2.80 x 1024 atoms of silicon? 2) (In class) 3) How many oxygen atoms in each:A) NH4NO3B) C9H8O4C) O3D) C3H5(NO3)3 1 moles 2.80 x 1024 atoms = 4.65 moles 6.02 x 1025 atoms

  8. Ch10 HW#1 1 – 7 1) How many moles in 2.80 x 1024 atoms of silicon? 2) (In class) 3) How many oxygen atoms in each:A) NH4NO33B) C9H8O44C) O33D) C3H5(NO3)39 1 moles 2.80 x 1024 atoms = 4.65 moles 6.02 x 1025 atoms

  9. 4) How many molecules in 2.14 mol CO? 5) How many moles in 4.65 x 1024 molecules of NO2?

  10. 4) How many molecules in 2.14 mol CO? 5) How many moles in 4.65 x 1024 molecules of NO2? 6.02 x 1023 molecules 2.14 mol CO = 1.29 x 1024 molecules 1 mol CO

  11. 4) How many molecules in 2.14 mol CO? 5) How many moles in 4.65 x 1024 molecules of NO2? 6.02 x 1023 molecules 2.14 mol CO = 1.29 x 1024 molecules 1 mol CO 4.63 x 1024 molecules 1 moles = 7.72 moles 6.02 x 1023 molecules

  12. 6) Gram molecular mass A. C2H6 B. PCl3 C. C3H7OH D. N2O5

  13. 6) Gram molecular mass A. C2H6 B. PCl3 C. C3H7OH D. N2O5 1 P @ 31.0 = 31.0 2 C @ 12.0 = 24.0 3 Cl @ 35.5 = 106.5 6 H @ 1.0 = 6.0 137.5 g/mol 30.0 g/mol

  14. 6) Gram molecular mass A. C2H6 B. PCl3 C. C3H7OH D. N2O5 1 P @ 31.0 = 31.0 2 C @ 12.0 = 24.0 3 Cl @ 35.5 = 106.5 6 H @ 1.0 = 6.0 137.5 g/mol 30.0 g/mol 2 N @ 14.0 = 28.0 3 C @ 12.0 = 36.0 5 O @ 16.0 = 80.0 8 H @ 1.0 = 8.0 108.0 g/mol 10 @ 16.0 = 16.0 60.0 g/mol

  15. 7) Gram Formula Mass A. Sr(CN)2 B. NaHCO3 C. Al2(SO3)3

  16. 7) Gram Formula Mass A. Sr(CN)2 B. NaHCO3 C. Al2(SO3)3 1 Sr @ 87.6 = 87.6 2 C @ 12.0 = 24.0 2 N @ 14.0 = 28.0 139.6 g/mol

  17. 7) Gram Formula Mass A. Sr(CN)2 B. NaHCO3 C. Al2(SO3)3 1 Sr @ 87.6 = 87.6 1 Na @ 23.0 = 23.0 2 C @ 12.0 = 24.0 1 H @ 1.0 = 1.0 2 N @ 14.0 = 28.0 1 C @ 12.0 = 12.0 3 O @ 16.0 = 48.8 139.6 g/mol 83.8 g/mol

  18. 7) Gram Formula Mass A. Sr(CN)2 B. NaHCO3 C. Al2(SO3)3 1 Sr @ 87.6 = 87.6 1 Na @ 23.0 = 23.0 2 C @ 12.0 = 24.0 1 H @ 1.0 = 1.0 2 N @ 14.0 = 28.0 1 C @ 12.0 = 12.0 3 O @ 16.0 = 48.8 139.6 g/mol 83.8 g/mol 2 Al @ 27.0 = 54.0 3 S @ 32.1 = 96.3 9 O @ 16.0 = 144.0 294.3 g/mol

  19. Ch10.2 – Mole/Mass Conversions Ex 1) How many grams are in 7.20 mol of dinitrogen trioxide? Ex 2) How many grams are in 3.41 mol of calcium oxide? Ex 3) Find the number of moles in 92.81g of Iron (III) Oxide?

  20. Ch10.2 – Mole/Mass Conversions Ex 1) How many grams are in 7.20 mol of dinitrogen trioxide? Ex 2) How many grams are in 3.41 mol of calcium oxide? 7.20 mol N2O3 76.0 grams N2O3 = 547 grams N2O3 1 mol N2O3 2 N @ 14.0 = 28.0 3 O @ 16.0 = 48.0 76.0 g/mol = 191 grams CaO Ex 3) Find the number of moles in 92.81g of Iron (III) Oxide? = .581 Moles

  21. HW#8) Find the mass of each: 0.720 mol Be b) 2.40 mol N2 (finish c, d) HW#9) Find # of moles in each: b) 0.000264g Li2HPO4 (finish #9) Ch 10 HW#2 8, 9

  22. Ch3 X.C. Average Density of Earth. Given: DiameterE = 12,756 km MassE = 5.98x1024 kg VolumeΘ= 4/3 πr3 DiameterE12756 km 2 2 VolumeE = 4/3.πr3 = 4/3.π(637,800,000 cm)3 = 1.09x1027 cm3 MassE = 5.98 x 1024 kg 5.98 x 10 27 g m 5.98 x 1027g V 1.09 x 1027 cm3 RadiusE = = = 6378 km = 637,800,000 cm D= = = 5.50 g/cm3

  23. Ch10 HW#2 8 – 9 8c) Convert to mass: 10.0 mol Cr d) 3.32 mol K

  24. Ch10 HW#2 8 – 9 8c) Convert to mass: 10.0 mol Cr 52.0g Cr 1 mol Cr = 520g Cr d) 3.32 mol K 39.1 g K 1 mol K = 130 g K

  25. Ch10 HW#2 8 – 9 8c) Convert to mass: 10.0 mol Cr 52.0g Cr 1 mol Cr = 520g Cr d) 3.32 mol K 39.1 g K 1 mol K = 130 g K 9) Find moles a) 5.00g H2 c) 72.0g Ar d) 3.70x10 -1 g

  26. Ch10 HW#2 8 – 9 8c) Convert to mass: 10.0 mol Cr 52.0g Cr 1 mol Cr = 520g Cr d) 3.32 mol K 39.1 g K 1 mol K = 130 g K 9) Find moles a) 5.00g H2 1 mol H2 2.0 g H2 = 2.5 mol H2 c) 72.0g Ar 1 mol Ar 39.9g Ar = 1.80 mol Ar d) 3.70x10 -1 g 1 mol B 10.8g B =

  27. Ch10.3 – Using the Mole Ex) What is the mass of 3.01x1023 atoms of Carbon? Ex) What is the mass of 12.04x1023 molecules of oxygen? Ex) How many molecules are there in 63.8g of ethanol, CH3OH? Ch10 HW #3 (10-12)

  28. Ch10.3 – Using the Mole Ex) What is the mass of 3.01x1023 atoms of Carbon? 3.01x1023 atoms C 1 mol C 12.0 g C 6.02x1023 atoms C 1 mol C = 6.00g C Ex) What is the mass of 12.04x1023 molecules of oxygen? 12.04x1023 molecules O2 1 mol O2 32.0g O2 6.02x1023molec. O2 1 mol O2 = 64.0g O2 Ex) How many molecules are there in 63.8g of ethanol, CH3OH? 63.8g CH3OH 1 mol CH3OH 6.02 x 1023 molecules CH3OH 32.0g CH3OH 1 mol CH3OH = 1.20 x 1024 molecules CH3OH Ch10 HW #3 (10-12)

  29. Lab10.1 – Molar Mass - due tomorrow - Ch10 HW#3 due at beginning of period

  30. Ch10 HW #3 10 – 12 10) What is the mass of 2.11 x 1024 molecules of sulfur dioxide? 2.11 x 1024 molecules SO2 1 S @ 32.1 = 32.1 2 0 @ 16 = 32.0 64.1 g/mol

  31. 10) What is the mass of 2.11 x 1024 molecules of sulfur dioxide? 2.11 x 1024 molecules SO2 1 moles SO2 64.1g SO2 = 224g SO2 6.02 x 1023 molecules SO2 1 moles SO2 1 S @ 32.1 = 32.1 2 0 @ 16 = 32.0 64.1 g/mol

  32. 11) What is the mass of 1.0 x 1022 molecules of iodine? 1.0 x 1022 molecules I2 2 I @ 126.9 = 253.8 g/mol

  33. 11) What is the mass of 1.0 x 1022 molecules of iodine? 1.0 x 1022 molecules I2 1 moles I2 253.8g I2 = 4.22g I2 6.02 x 1023 molecules I2 1 moles I2 2 I @ 126.9 = 253.8 g/mol

  34. 12) How many molecules is 126.7g of sucrose? 126.7g C6H12O6 6 C @ 12.0 = 72.0 12 H @ 1.0 = 12.0 6 O @ 16.0 = 96.0 180.0 g/mol

  35. 12) How many molecules is 126.7g of sucrose? 6.02 x 1023 molecules C6H12O6 1 mol C6H12O6 126.7g C6H12O6 180.0g C6H12O6 1 mol C6H12O6 = 4.23 x 1023 molecules C6H12O6 6 C @ 12.0 = 72.0 12 H @ 1.0 = 12.0 6 O @ 16.0 = 96.0 180.0 g/mol

  36. Ch10.4 – Volume of a Mole of Gas Volumes of gases can change a lot, if temp or pressure change. Standard temperature and pressure: (STP) Temp: 0°C (273K) Pressure: 101.3 kPa(kiloPascals)or 1 atmosphere At STP, 1 mole of any gas occupies a volume of 22.4 Liters. 1 mol 22.4 L 22.4 L 1 mol or

  37. Ch10.4 – Volume of a Mole of Gas Volumes of gases can change a lot, if temp or pressure change. Standard temperature and pressure: (STP) Temp: 0°C (273K) Pressure: 101.3 kPa(kiloPascals)or 1 atmosphere At STP, 1 mole of any gas occupies a volume of 22.4 Liters. Ex 1) What is the volume of 0.600 mol of SO2 gas at STP? 1 mol 22.4 L 22.4 L 1 mol or

  38. Ch10.4 – Volume of a Mole of Gas Volumes of gases can change a lot, if temp or pressure change. Standard temperature and pressure: (STP) Temp: 0°C (273K) Pressure: 101.3 kPa(kiloPascals)or 1 atmosphere At STP, 1 mole of any gas occupies a volume of 22.4 Liters. Ex 1) What is the volume of 0.600 mol of SO2 gas at STP? 1 mol 22.4 L 22.4 L 1 mol or 0.600 mol SO2 22.4 L SO2 = 13.4 L SO2 1 mol SO2

  39. Ex 2) Determine the # of moles in 33.6 L of He gas at STP: Ex 3) The density of a gaseous compound of C and O is 1.964 g/L at STP. Determine the gram formula mass. Is it CO or CO2? CO: 1 C @ 12.0 = 12.0 1 O @ 16.0 = 16.0 20.0 g/mol CO2: 1 C @ 12.0 = 12.0 2 O @ 16.0 = 32.0 44.0 g/mol

  40. Ex 2) Determine the # of moles in 33.6 L of He gas at STP: Ex 3) The density of a gaseous compound of C and O is 1.964 g/L at STP. Determine the gram formula mass. Is it CO or CO2? 1.964g 1 L 1 mol He = 1.50 mol He 22.4 L He CO: 1 C @ 12.0 = 12.0 1 O @ 16.0 = 16.0 20.0 g/mol CO2: 1 C @ 12.0 = 12.0 2 O @ 16.0 = 32.0 44.0 g/mol

  41. Ex 2) Determine the # of moles in 33.6 L of He gas at STP: Ex 3) The density of a gaseous compound of C and O is 1.964 g/L at STP. Determine the gram formula mass. Is it CO or CO2? 1.964g 1 L 1 mol He = 1.50 mol He 22.4 L He 1.964g 1 L 22.4 L = 44.0 g/mol 1 mol CO: 1 C @ 12.0 = 12.0 1 O @ 16.0 = 16.0 20.0 g/mol CO2: 1 C @ 12.0 = 12.0 2 O @ 16.0 = 32.0 44.0 g/mol

  42. Ex4) 10.4g of dry ice, CO2 , is allowed to sublime into a gas. If the gas is brought to STP, what volume does it occupy? Ex5) 1.13x1022 molecules of hydrogen gas occupy what volume at STP?

  43. Ex4) 10.4g of dry ice, CO2 , is allowed to sublime into a gas. If the gas is brought to STP, what volume does it occupy? = 5.29L CO2 Ex5) 1.13x1022 molecules of hydrogen gas occupy what volume at STP?

  44. Ex4) 10.4g of dry ice, CO2 , is allowed to sublime into a gas. If the gas is brought to STP, what volume does it occupy? = 5.29L CO2 Ex5) 1.13x1022 molecules of hydrogen gas occupy what volume at STP? = .420L H2 Ch 10 HW #4 13-18

  45. Ch 10 HW#4 13-18 ( XC for correct #16 ) 13) 3 balloons each contain the same # of molecules of 3 different gases @ STP. Same mass? Same volume? CO2 O2 H2

  46. Ch 10 HW#4 13-18 ( XC for correct #16 ) 13) 3 balloons each contain the same # of molecules of 3 different gases @ STP. Same mass? Same volume? Diff mass Same volume CO2 O2 H2

  47. 14) Volume @ STP a) 3.20x10-3 mol CO2 b) 0.960 mol CH4 c) 3.70 mol N2 15) At STP, how many moles? a) 67.2L SO2 b) 0.880L He c) 1.00x103L C2H6

  48. 14) Volume @ STP a) 3.20x10-3 mol CO2 22.4L CO2 1 mol CO2 = .0717l CO2 b) 0.960 mol CH422.4L CH4 1 mol CH4 = 21.5L CH4 c) 3.70 mol N222.4L N2 1 mol N2 = 82.9L N2 15) At STP, how many moles? a) 67.2L SO2 1 mol SO2 22.4 L SO2 = b) 0.880L He 1 mol He 22.4 L He = c) 1.00x103L C2H6 1 mol C2H6 22.4 L C2H6 =

  49. 14) Volume @ STP a) 3.20x10-3 mol CO2 22.4L CO2 1 mol CO2 = .0717l CO2 b) 0.960 mol CH422.4L CH4 1 mol CH4 = 21.5L CH4 c) 3.70 mol N222.4L N2 1 mol N2 = 82.9L N2 15) At STP, how many moles? a) 67.2L SO2 1 mol SO2 22.4 L SO2 = 3.00 mol SO2 b) 0.880L He 1 mol He 22.4 L He = .0393 mol He c) 1.00x103L C2H6 1 mol C2H6 22.4 L C2H6 = 44.6 mol C2H6

  50. 16) AT STP what volume does 12.2g fluorine gas occupy? 12.2 g F2 1 mol F2 22.4 L F2 38.0 g F2 1 mol F2 = 17) 13.0 x 1024 molecules of Argon occupy what volume at STP? 13.0 x 1024 molecules Ar 1 mol Ar 22.4 L Ar 6.02 x 1023 1 mol Ar = molecules Ar

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