1. The Mole Chapter 10

3. How do you measure? Often measure something by one of three different methods-  by counting  by mass  by volume

4. How about them apples By count: 1 dozen = 12 apples By mass: 1 dozen = 2.0 kg of apples By volume: 1 dozen = 0.2 bushels To do this you must use conversion factors

5. Practice Problems If 0.20 bushel is 1 dozen apples & a dozen apples has a mass of 2.0 kg, what is the mass of 0.50 bushel of apples? Assume 2.0 kg of apples is 1 dozen and that each apple has 8 seeds. How many apple seeds are in 14 kg of apples?

6. What is a mole? 6.02 x10 23  also known as Avogadro’s number 602,000,000,000,000,000,000,000 Considers the very small size of atoms Helps with the conversion of units

7. But What is a Mole??? 6.02x10 23 representative particles are in each and every mole SI unit of measuring the amount of a substance

8. Representative particle Atoms Molecules Formula units A mole of any substance contains Avogadro’s number of representative particles

9. Converting Number of particles to moles Equation This equation can be placed in a unit conversion to find the number of particles

11. Practice Problem Magnesium is a light metal used in the manufacture of aircraft, automobile wheels, tools and garden furniture. How many moles of magnesium is 1.25 * 10 23 atoms of magnesium?

12. Converting Moles to Number of Particles Determining how many atoms are in one mole of a compound This number is discovered from the formula:

13. Molecules and Atoms How many moles are in one CO 2 molecule? A mole of CO 2 of contains 1 Avogadro’s number of carbon dioxide molecules However, there are 3 atoms in every 1 molecule of carbon dioxide  So, there are 3 moles worth of atoms in every 1 moles worth of carbon dioxide molecules

14. Converting Moles to Number of Particles To find the number of atoms, molecules, representative particles in a mole of a compound, you must first determine the number of representative particles, then you can use the following equation

15. Practice Problems Propane is a gas used for cooking & heating. How many atoms are in 2.12 mole of propane (C 3 H 8 )?

16. The mass of a mole of an element The atomic mass of a single atom is expressed as atomic mass units Atomic mass units is the atomic mass expressed in grams What is the atomic mass of krypton?

18. Molar Mass of an element Mass of one mole of an element Example:  1 mole of gold weighs 196 g  What is the mass of 1 mole of Magnesium?

20. Pop Quiz What is the molar mass of oxygen? What is the molar mass of carbon? What is the molar mass of hydrogen?

21. Molar Mass To calculate the molar mass of a compound:  Find the number of grams of each element in one mole of the compound.  Then add the masses of the elements in the compound Applies to ionic & molecular compounds Ex: Carbon Dioxide (CO 2 ) 44 g/mol

22. Finding Molar Mass of Sulfur Trioxide Determine how many atoms of each element are in the compound Add up the masses of all the atoms

23. Mole-Mass and Mole-Volume Relationships 10.2

24. Mole to Mass Relationship Molar Mass = mass of 1 mole of a substance We can determine the mass of a substance through the number of moles it contains Must use a conversion factor

25. Practice Problem Determine the mass of 5 moles of NaCl. Use the following equation

26. Converting Mass to Moles Given a mass Convert to moles

28. The Mole-Volume Relationship Avagadro’s hypothesis:  Equal volumes of gases at the same temperature and pressure contain equal number of particles Change in temperature or pressure will change the volume Figure 10.9 In each container, the volume occupied by the gas molecules is small compared with the container ﾕ s volume, so the molecules are not tightly packed. a. The molecules in this container are small. b. This container can accommodate the same number of larger molecules.

29. Change in Temperature

30. Standard Temperature & Pressure (STP) We usually measure volume at STP  Temperature: 0 o C  Pressure: 101.3 kPa or 1 atm At STP, 1 mol or 6.02x10 23 rep particles, of any gas occupies a volume of 22.4L 22.4L = molar Volume

31. Calculating Volume at STP Molar volume can be used to convert the known number of moles to the volume of a gas at STP

33. Calculating Molar Mass from Density Density of a gas at STP and the molar volume at STP (22.4L/mol) can be used to calculate the molar mass of a gas

35. The Mole Road Map

36. Percent Composition and Chemical Formulas 10.3

37. Percent Composition Relative amounts of elements in a compound  Also known as the percent by mass of each element in the compound We can use a simple formula to determine % composition

38. Percent Composition from Mass Data Use of analytical procedures to determine the relative masses of each element in the compound and calculate the percent composition

40. Percent Composition from the Chemical Formula If you know the formula you can calculate the percent composition using the following Figure 10.14 The percent composition of water is always the same regardless of the volume of the water sample. A sample of water is always 11.1% H and 88.9% O by mass.

42. Percent Composition as a Conversion Factor Use percent composition to calculate the number of grams of any element in a specific mass of a compound Multiply mass of compound by a conversion factor based on the percent composition

43. Practice Problem How much C & H are in 82.0 g of propane You found that propane is 81.8% C and 18% H. That means that in a 100-g sample of propane, you would have 81.8 g of C and 18 g of H. You can use the ratio to calculate the mass of carbon contained in 82.0 g of propane (C 3 H 8 ).

44. Empirical Formula Lowest whole number ratio of the atoms of the elements in a compound Example:  H 2 O 2 or Hydrogen Peroxide  The ratio is 1:1 even though there are two atoms of each element in the compound

45. Calculating Empirical Formula Convert your percent and express as moles Convert from grams to moles using your mole ratio Divide each by the lower number of moles

48. Molecular Formula Either the same as its empirical formula Or a simple whole number multiple of its empirical formula