chemical quantities all roads lead to the mole chemical quantities measuring donuts: 1 dozen = 12...
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CHEMICAL QUANTITIES
All Roads Lead to the Mole
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Chemical Quantities
Measuring donuts:• 1 dozen = 12 donuts (count) • 1 dozen = 500 g donuts (mass)• 1 dozen = 1 box donuts
(volume)Measuring steam (H2O gas):
• 1 mole = 6.02 x 1023 H2O molecules (count)
• 1 mole = 18.0 g H2O (mass)
• 1 mole = 22.4 L H2O (volume) at STP
Dozen: Baker as Mole: Chemist
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Count Amedeo Avogadro
• 1776-1856• Lawyer who became interested in
math and physics• Discovered that equal volumes
of different gases contained an equal number of particles.
• 9 years after his death, Joseph Loschmidt determined a constant and named it after Avogadro.
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AVOGADRO’S CONSTANT= 6.02 x 1023
Not to be confused with the delicious
fruit
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AVOGADRO’S CONSTANT= 6.02 x 1023
• 1 mole = 6.02 x 1023 particles• 1 mole = molar mass (grams)• 1 mole (of a gas at STP) = 22.4 L
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The mole is to chemists
as
the dozen is to bakers.
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Believe it or not, students all over the country celebrate National Mole Day!
National Mole Day Foundation, INC.
Mole Day
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5 Pound Bag of Sugar contains 6.6 moles Of C12H22O11 1 Liter bottle of Water contains 55.5 moles H206.02 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. 6.02 x 1023 Watermelon Seeds: Would be found inside a melon slightly larger than the moon.6.02 x 1023 Pennies: Would make at least 7 stacks that would reach the moon.6.02 x 1023 Donut Holes: Would cover the earth and be 5 miles (8 km) deep.
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MassVolume
R.P.Molecules
Atoms
Formula Units
Ions
Draw on NOTETAKERS (and pass out flow Mole Map)
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Types of Representative Particles
• Molecules (break down into atoms)
• Atoms
• Formula Units (break down into ions)
• Ions
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Naming Representative Particles
Examples: Name the representative particle for each substance given. For each molecule, state how many atoms are present. For each formula unit, state how many ions make up the ionic compound.
H+:
Cl2:
C2H6:
Cu(NO3)2:
Al:
NaCl:
ION
MOLECULE – 2 ATOMS per molecule
MOLECULE – 8 ATOMS
FORMULA UNIT – 3 IONS per Form.U.
ATOM
FORMULA UNIT – 2 IONS per Form.U.
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WS: Representative Particles
Do WS #1-20
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Mole R.P. Calculations
1 mole = Avogadro’s Number = 6.02 x 1023 R.P.’s
R.P.mol 1
R.P.106.02 23
R.P.106.02
mol 123
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R.P. Example 1:How many moles are in 1.4 x 1022 molecules of H2O?
O Hmolecules1002.6
O Hmol 1O Hmolecules104.1
223
2222
OH mol 023.0 2
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R.P. Example 2:How many representative particles are in 2.6 mol CO2?
2
223
2
CO mol 1
CO molecules 106.02CO mol 6.2
224 CO molecules 106.1
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R.P. Example 3:How many atoms are in 5.2 mol CO2?
22
223
2
CO molecule 1
atoms3
CO mol 1
CO molecules106.02CO mol 2.5
atoms104.9 24
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DO WS:
The Mole and Avogadro’s Number
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MOLAR MASS
The molar mass is the mass, in grams,
of one mole (6.02 1023 particles) of an
element (ion), a covalent molecule or a
formula unit.
molar mass (MM) gram atomic mass (gam)molecular weight (MW) gram molecular mass (gmm)formula mass (FM) gram formula mass (gfm)formual weight (FW)
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Molar Mass … a.k.a. Molecular Weight (MW)
molar mass = mass of 1 mole of substance
Molar mass can be determined by adding up the atomic masses from the periodic table (atomic mass goes to 2 decimal places).
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MW Example 1:
Find the MW of CH4.
= 1C + 4H = 12.01 + 4(1.01) = 16.05 g CH4/mol CH4
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MW Example 2:
Find the MW of Mg(OH)2.
=Mg + 2O + 2H=24.31 + 2(16.00) + 2(1.01)=58.33 g Mg(OH)2 /mol Mg(OH)2
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MW Example 3:
Find the MW of MgSO4∙7H2O.
=Mg + S + 4O + 7(H2O)
=24.31 + 32.07 + 4(16.00) + 7(1.01+1.01+16.00)
= 246.52 g MgSO4∙7H2O /mol MgSO4∙7H2O
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Calculations:
Use Mole Map to help calculate
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Mole Mass Calculations
1 mole = molar mass (MW) in grams
Massmol 1
(g) massmolar
(g) massmolar
mol 1
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Mass Example 1:
How many grams are in 7.20 moles of dinitrogen trioxide?
MW of N2O3 = 2N + 3O = 2(14.01) + 3(16.00) =76.02 g/mol
1 mole = 76.02 g N2O3
dinitrogen trioxide = N2O3
3232
3232 ON g547ON mol 1.00
ON g 02.76ON mol20.7
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Mass Example 2:
Find the number of moles in 92.2 g of iron(III) oxide.
MW of Fe2O3 = 2Fe + 3O = 2(55.85) + 3(16.00) =159.70 g/mol
1 mole = 159.70 g Fe2O3
iron(III) oxide = Fe2O3
3232
3232 O Femol577.0O Feg 159.70
O Femol 1O Feg2.92
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Practice Worksheet
Do #1-10 on Mole and Mass WS
Make sure you write out all work and include all units!!
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Mole Volume Calculations
1 mole = 22.4 L of gas at STP
STP = standard temperature and pressure (0 °C & 1 atm)
Volumemol 1
L 22.4
L 22.4
mol 1
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Volume Example 1:
Determine the volume, in liters, of 0.600 mol of SO2 gas at STP.
2
22
SO mol 1
SO L4.22SO mol600.0
2SO L4.13
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Volume Example 2:
Determine the number of moles in 33.6 L of He gas at STP.
He L22.4
Hemol 1 He L3.63
He mol 50.1
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Density
density = mass / Volume
When given the density of an unknown gas, one can multiply by the molar volume to find the MW.
The MW can allow for identification of the gas from a list of possibilities.
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Density Example (part A):
The density of an unknown gas is 2.054 g/L at STP. (a) What is the molar mass?
massmolar memolar voludensity
1mol
L4.22
L
2.054g g/mol 01.46
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Density Example (part B):
The density of an unknown gas is 2.054 g/L. (b) Identify the gas as either nitrogen, fluorine, nitrogen dioxide, carbon dioxide, or ammonia.
MW = 46.01 g/mol (from part a)
Nitrogen = N2 = 2(14.01) = 28.02 g/mol
Fluorine = F2 = 2(19.00) = 38.00 g/mol
Nitrogen dioxide = NO2 = 14.01 + 2(16.00) = 46.01 g/mol
Carbon dioxide = CO2 = 12.01 + 2(16.00) = 44.01 g/mol
Ammonia = NH3 = 14.01 + 3(1.01) = 17.04 g/mol
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Mixed Mole Conversions
1 mole = 6.02 x 1023 RP’s =
MW = 22.4 L of gas @STP
All Roads Lead to the Mole.
Always convert to units of moles first when converting between grams, liters, and representative particles.
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Mixed Mole Example 2:
How many atoms are in 22.0 g of water?
242.20 10 atoms
22.0 g H 2O❑ ×
1 mole H 2O18.02 g H2 O
×6.02 ×10 23 molec . H2O1 mole H 2O
×3 atoms1 molec . H2O
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Mixed Mole Example 1:
How many carbon atoms are in a 50.0-carat diamond that is pure carbon? Fifty carats is the same as 10.0 g.
C mol 1
C atoms 1002.6
C g 12.01
C mol 1C g 0.10 23
C atoms 1001.5 23
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Extra questions to review concepts
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What is the mass of 3.7 moles of NaCl?
a) 15.8 gb) 58.5 gc) 220 gd) 6.02 x 1023 g
NaCl mol 1
NaCl g 44.58NaCl mol7.3
NaCl g 23.216
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How many moles are in 152 g of water?
a) 0.118 molb) 8.44 molc) 2736 mold) 6.02 x 1023 mol
O Hg 02.18
O Hmol 1
1
O Hg 152
2
22
O Hmol 44.8 2