Ch 10 chemical quantities
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Ch. 10 Chemical Quantities. 3 Methods of Measuring. Counting Mass Volume. Example 1. If 0.20 bushel is 1 dozen apples, and a dozen apples has a mass of 2.0 kg, what is the mass of .050 bushel of apples?. Example 1. Count: 1 dozen apples = 12 apples Mass: 1 dozen apples = 2.0 kg apples

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Ch. 10 Chemical Quantities

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Ch 10 chemical quantities

Ch. 10 Chemical Quantities


3 methods of measuring

3 Methods of Measuring

  • Counting

  • Mass

  • Volume


Example 1

Example 1

  • If 0.20 bushel is 1 dozen apples, and a dozen apples has a mass of 2.0 kg, what is the mass of .050 bushel of apples?


Example 11

Example 1

  • Count: 1 dozen apples = 12 apples

  • Mass: 1 dozen apples = 2.0 kg apples

  • Volume: 1 dozen apples = 0.20 bushels

    apples

    Conversion Factors:

  • 1 dozen2.0 k.g1 dozen

    12 apples 1 dozen 0.20 bushels


Example 12

Example 1

  • 0.50 bushel x 1 dozen x 2.0 kg =

    0.20 bushel 1 dozen

    = 5.0 kg


Avogadro s number

Avogadro’s Number

  • Named after the Italian scientist Amedo Avogadro di Quaregna

  • 6.02 x 10 23


Mole mol

Mole (mol)

  • 1 mol = 6.02 x 10 23 representative particles

  • Representative particles: atoms, molecules ions, or formula units (ionic compound)


Mole mol1

Mole (mol)

  • Moles= representative x 1 mol

    particles 6.02 x 10 23


Example 2 atoms mol

Example 2 (atoms  mol)

  • How many moles is 2.80 x 10 24 atoms of silicon?


Example 2

Example 2

  • 2.80 x 10 24 atoms Si x 1 mol Si

    6.02 x 10 23 atoms Si

    = 4.65 mol Si


Example 3 mol molecule

Example 3 (mol  molecule)

  • How many molecules of water is 0.360 moles?


Example 3

Example 3

  • 0.360 mol H2O x 6.02 x 10 23 molecules H2O1 mol H2O

    =2.17 molecules H2O


The mass of a mole of an element

The Mass of a Mole of an Element

  • The atomic mass of an element expressed in grams = 1 mol of that element = molar mass

Molar mass S

Molar mass Hg

Molar mass C

Molar mass Fe


Ch 10 chemical quantities

6.02 x 10 23 atoms S

6.02 x 10 23 atoms Hg

6.02 x 10 23 atoms C

6.02 x 10 23 atoms Fe


Example 4 mol gram

Example 4 (mol  gram)

  • If you have 4.5 mols of sodium, how much does it weigh?


Example 4

Example 4

  • .45 mol Na x 23 g Na = 10.35 g Na = 1.0 x 10 2 g Na

    1 mol Na


Example 5 grams atoms

Example 5 (grams  atoms)

  • If you have 34.3 g of Iron, how many atoms are present?


Example 5

Example 5

  • 34.3 g Fe x 1 mol Fe x 6.02 x 10 23 atoms

    55.8 g Fe 1 mol Fe

    =3.70 x 10 23 atoms Fe


The mass of a mole of a compound

The Mass of a Mole of a Compound

  • To find the mass of a mole of a compound you must know the formula of the compound

  • H2O  H= 1 g x 2

    O= 16 g

    18 g = 1 mole = 6.02 x 10 23

    molecules


Example 6 gram mol

Example 6 (gram  mol)

  • What is the mass of 1 mole of sodium hydrogen carbonate?


Example 6

Example 6

  • Sodium Hydrogen Carbonate = NaHCO3

  • Na=23 g

  • H=1 g

  • C=12 g

  • O=16 g x3

  • 84 g NaHCO3 = 1 mol NaHCO3


Mole volume relationship

Mole-Volume Relationship

  • Unlike liquids and solids the volumes of moles of gases at the same temperature and pressure will be identical


Avogadro s hypothesis

Avogadro’s Hypothesis

  • States that equal volumes of gases at the same temperature and pressure contain the same number of particles

  • Even though the particles of different gases are not the same size, since the gas particles are spread out so far the size difference is negligible


Standard temperature and pressure stp

Standard Temperature and Pressure (STP)

  • Volume of a gas changes depending on temperature and pressure

  • STP= 0oC (273 K)

    101.3 kPa (1 atm)


Standard temperature and pressure stp1

Standard Temperature and Pressure (STP)

  • At STP, 1 mol = 6.02 X 1023 particles = 22.4 L of ANY gas= molar volume


Conversion factors

Conversion Factors

  • AT STP

  • 1 mol gas22.4 L gas

    22.4 L gas 1 mol gas


Example 7

Example 7

  • At STP, what volume does 1.25 mol He occupy?


Example 71

Example 7

  • 1.25 mol He x 22.4 L He = 28.0 L He

    1 mol He


Example 8

Example 8

  • If a tank contains 100. L of O2 gas, how many moles are present?


Example 81

Example 8

  • 100. L O2 X 1 mol O2 = 4.46 mol O2

    22.4 L O2


Calculating molar mass from density

Calculating Molar Mass from Density

  • The density of a gas at STP is measured in g/L

  • This value can be sued to determine the molar mass of gas present


Example 9

Example 9

  • A gaseous compound of sulfur and oxygen has a density of 3.58 g/L at STP. Calculate the molar mass.


Example 91

Example 9

  • 1 mol gas x 22.4 L gas X 3.58 g gas =

    1 mol gas 1 L gas

    Molar Mass= 80.2 g


Percent composition

Percent Composition

  • The relative amounts of the elements in a compound

  • These percentages must equal 100


Percent composition1

Percent Composition

  • %element = mass of element x 100

    mass of compound


Example 10

Example 10

  • Find the percentage of each element present in Al2 (CO3)3


Example 101

Example 10

  • Al2(CO3)3

  • Al= 27 g x 2 = 54 g / 234 g x 100=23%

  • C= 12 g x 3 = 36 g/ 234 g x 100= 15%

  • O = 16 g x 9 = 144 g / 234 g x 100=62%

    234 gAl2(CO3)3


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