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The Mole

The Mole. Unit 5. Formula Mass. Formula mass - also called: formula mass molecular mass molecular mass formula weight formula weight molecular weight molecular weight molar mass molar weight the mass of one mole of a compound, atom or ion. (units: _ g _ ) mol.

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The Mole

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  1. The Mole Unit 5

  2. Formula Mass • Formula mass - also called: formula mass molecular mass molecular mass formula weight formula weight molecular weight molecular weight molar mass molar weight the mass of one mole of a compound, atom or ion. (units: _g_ ) mol

  3. Formula Mass: Example: Calculate the formula mass of the following: I Do: carbon tetrachloride Formula: CCl4 1 C: 12.011 g/mol 4 Cl: 4 x 35.45 g/mol = 141.8 g/mol Total mass: 153.81 g/mol

  4. Formula Mass Example: Find the formula mass of each of the following: We Do: arsenic trichloride: Formula: AsCl3 1 As: 74.922 g/mol 3 Cl: 3 x 35.45 g/mol = 106.35 g/mol Total mass: 181.27 g/mol

  5. Formula Mass Example: Find the formula mass of each of the following: You Do: potassium sulfide Formula: K2S 2 K: 2 x 39.098 g/mol = 78.196 g/mol 1 S: 32.066 g/mol Total mass: 110.262 g/mol

  6. Measuring Matter There are three ways to measure matter: • By counting representativeparticles: atoms – element molecules- covalent compound formula units- ionic compound ions – anything with a charge . Al, Na, S, etc PCl3,O2, CO2 AlCl3,K2O, Ba3P2 PO32-,K1+

  7. 2. By mass - in grams 3. By volume - in liters for gases (at STP)

  8. Measuring Matter 1 mole of a compound = formula mass (in grams) 1 mole of a compound = 6.02 x 1023 representative particles 1 mole of a gas (STP) = 22.4 liters The mole is the link between grams, the number of representative particles and liters! Remember: There are 4 different types of Representative Particles Atoms Formula units Molecules Ions

  9. Identify the type of Representative Particle • NaCl • F2 • NH4+1 • CS2 • H2O • Be • CsF Formula Units Molecules Ions Molecules Molecules Atoms Formula Units

  10. Mole Road Map

  11. Mole Practice: One Step Conversions: Remember to show all work using dimensional analysis. I Do: How many moles are present in a tank of gas that contains 55.60 Liters? Conversion Factors: 1 mole = formula mass 1 mole or g g 1 mole 1 mole = 6.022 x 1023 1 mole or6.022 x 1023 particles 6.022 x 1023 1 mole 1 mole = 22.4 Liters gas 1 moleor 22.4 L 22.4 L 1 mole = 2.48 moles of gas 55.60 Liters Make sure to round the final Answer to the 100th place. Only the final answer!

  12. Mole Practice: One Step Conversions: Remember to show all work using dimensional analysis. We Do: How many moles are in 18.0 grams of sugar (C6H12O6)? Conversion Factors: 1 mole = formula mass 1 mole or g g 1 mole 1 mole = 6.022 x 1023 1 mole or6.022 x 1023 particles 6.022 x 1023 1 mole 1 mole = 22.4 Liters gas 1 moleor 22.4 L 22.4 L 1 mole 18.0 g C6H12O6 Make sure to round the final Answer to the 100th place. Only the final answer! Add Masses of 6C + 12H + 6O You must use all the Numbers from the Periodic Table

  13. Mole Practice: One Step Conversions: Remember to show all work using dimensional analysis. You Do: What is the mass in grams of 4.50 moles of barium sulfide? Conversion Factors: 1 mole = formula mass 1 mole or g g 1 mole 1 mole = 6.022 x 1023 1 mole or6.022 x 1023 particles 6.022 x 1023 1 mole 1 mole = 22.4 Liters gas 1 moleor 22.4 L 22.4 L 1 mole Add Masses of 1 Ba + 1 S You must use all the Numbers from the Periodic Table 4.50 mol BaS Make sure to round the final Answer to the 100th place. Only the final answer!

  14. Two and Three Step Conversions I Do: What is the mass in grams of 5.02 x 1024 formula units of potassium phosphate? Conversion Factors: 1 mole = formula mass 1 mole or g g 1 mole 1 mole = 6.022 x 1023 1 mole or6.022 x 1023 particles 6.022 x 1023 1 mole 1 mole = 22.4 Liters gas 1 moleor 22.4 L 22.4 L 1 mole 5.02x1024 Formula units K3PO4 = 1117.98 g K3PO4

  15. Two and Three Step Conversions We Do: How many molecules are in 198.5 grams of sodium chloride? Conversion Factors: 1 mole = formula mass 1 mole or g g 1 mole 1 mole = 6.022 x 1023 1 mole or6.022 x 1023 particles 6.022 x 1023 1 mole 1 mole = 22.4 Liters gas 1 moleor 22.4 L 22.4 L 1 mole = 2.04x1024 Formula Units NaCl 198.5g NaCl

  16. Two and Three Step Conversions You Do: How many Liters of gas is 3.21 x 1024 molecules of carbon monoxide? Conversion Factors: 1 mole = formula mass 1 mole or g g 1 mole 1 mole = 6.022 x 1023 1 mole or6.022 x 1023 particles 6.022 x 1023 1 mole 1 mole = 22.4 Liters gas 1 moleor 22.4 L 22.4 L 1 mole = 119.44 L CO 3.21x1024 Molecules CO

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