notes: 10.1-10.2 – chemical quantities (the mole / molar mass) all roads lead to the mole!!
TRANSCRIPT
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NOTES: 10.1-10.2 – Chemical Quantities
(The Mole / Molar Mass)
All Roads Lead to the
Mole!!
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What is a mole?
● A unit of measure used to count atoms, molecules, or ions
● A number: 6.02 x 1023
(Avogadro’s number)
● 1 mol = 6.02 x 1023 (conversion factor)
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Chemical Quantities – consider another word that means a #:
● Measuring doughnuts: a DOZEN!
1 dozen = 12 doughnuts (count)
1 dozen = 500 g doughnuts (mass)
1 dozen = 1 box doughnuts (volume)
● Measuring hydrogen (H2 gas): a MOLE!
1 mole = 6.02 x 1023 H2 molecules (count)
1 mole = 2.0 g H2 (mass)
1 mole = 22.4 L H2 (volume) at STP
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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
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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● 6.02 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 combined 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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How big is Avogadro's number? ● An Avogadro's number of soft drink cans would cover the surface of the earth to a depth of over 200 miles. ● If you spread Avogadro's number of unpopped popcorn kernels across the USA, the entire country would be covered in popcorn to a depth of over 9 miles. ● If we were able to count atoms at the rate of 10 million per second, it would take about 2 billion years to count the atoms in one mole. ● If you count out loud starting with the number "one" at the rate of one count every second, it may take you about 1,909,577,942,668,696 years to finish. This is roughly 960,000 times the estimated lifetime of our universe (assuming 20 Billion years). ● Using a Pentium 450 MHz CPU, it will still take about 4,243,506 years to finish this task. This is a period of time about a thousand times longer than the total span of our civilization.
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Why such a BIG number?
● because atoms, ions, molecules…are SO small!
● 5 Pound Bag of Sugar contains
6.6 moles of C12H22O11 molecules
● 1 Liter bottle of Water contains 55.5 moles H20 of water molecules
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MassVolume
R.P.Molecules
Atoms
Formula Units
Ions
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Types of Representative Particles:
● Molecules (breaks down into atoms)
● Atoms
● Formula Units (breaks down into ions)
● Ions
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Naming Representative Particles (R.P.s):
Pure Substance
Element Compound
Monatomic Polyatomic
Charged Neutral
ION ATOM
MOLECULE
ATOMS
Molecular Ionic
MOLECULE
ATOMS
FORMULA UNIT
IONS
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Naming Representative Particles (R.P.s):
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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Mole R.P. Calculations(particle #)
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 represented by
1.4 x 1022 molecules of H2O?
OH molecules1002.6
mol1OH molecules104.1
223
222
OH mol 023.0 2
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R.P. Example #2:How many molecules of CO2 are present 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 individual 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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Avogadro’s Number Practice Problems:
1) How many moles of magnesium are represented by 1.25 x 1023 atoms of magnesium?
ANSWER:
2) How many C3H8 molecules are in 2.12 mol of propane (C3H8)?
ANSWER:
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Avogadro’s Number Practice Problems:
1) How many moles of magnesium are represented by 1.25 x 1023 atoms of magnesium?
ANSWER: 0.208 mol Mg
2) How many C3H8 molecules are in 2.12 mol of propane (C3H8)?
ANSWER:
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Avogadro’s Number Practice Problems:
1) How many moles of magnesium are represented by 1.25 x 1023 atoms of magnesium?
ANSWER: 0.208 mol Mg
2) How many C3H8 molecules are in 2.12 mol of propane (C3H8)?
ANSWER: 1.28 x 1024 C3H8 molecules
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How about MOLES and MASS?
● when we measure out substances in the lab, it is not practical to count individual molecules…
● instead, we can use a balance to weigh out a certain amount…
● it is therefore useful to have a way to convert from moles to mass (and vice versa!)
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MOLAR MASS … a.k.a. Molecular Weight (MW)
● molar mass = mass of 1 mole of a substance
● Molar mass can be determined by adding up the atomic masses from the periodic table.
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Molar Mass Example #1:
• Find the molar mass of CH4.
= 1C + 4H
= 12.0 + 4(1.0)
= 16.0 g/mol
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Molar Mass Example #2:
• Find the molar mass of Mg(OH)2.
= Mg + 2O + 2H
= 24.3 + 2(16.0) + 2(1.0)
= 58.3 g/mol
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Molar Mass Example #3:
• Find the molar mass of MgSO4•7H2O.
= Mg + S + 4O + 7(H2O)
= 24.3 + 32.1 + 4(16.0) + 7(18.0)
= 246.4 g/mol
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Molar Mass Practice Problems:
● Determine the molar mass of the following
compounds:
1) H2O2
2) Carbon tetrabromide
3) (NH4)2CO3
4) Aluminum sulfate
5) Ca(NO3)2
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Molar Mass Practice Problems:
● Determine the molar mass of the following
compounds:
1) H2O2 : 34.0 g/mol
2) Carbon tetrabromide
3) (NH4)2CO3
4) Aluminum sulfate
5) Ca(NO3)2
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Molar Mass Practice Problems:
● Determine the molar mass of the following
compounds:
1) H2O2 : 34.0 g/mol
2) Carbon tetrabromide: 331.6 g/mol
3) (NH4)2CO3
4) Aluminum sulfate
5) Ca(NO3)2
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Molar Mass Practice Problems:
● Determine the molar mass of the following
compounds:
1) H2O2 : 34.0 g/mol
2) Carbon tetrabromide: 331.6 g/mol
3) (NH4)2CO3 : 96.0 g/mol
4) Aluminum sulfate
5) Ca(NO3)2
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Molar Mass Practice Problems:
● Determine the molar mass of the following
compounds:
1) H2O2 : 34.0 g/mol
2) Carbon tetrabromide: 331.6 g/mol
3) (NH4)2CO3 : 96.0 g/mol
4) Aluminum sulfate : 342.3 g/mol
Al2(SO4)3
5) Ca(NO3)2
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Molar Mass Practice Problems:
● Determine the molar mass of the following
compounds:
1) H2O2 : 34.0 g/mol
2) Carbon tetrabromide: 331.6 g/mol
3) (NH4)2CO3 : 96.0 g/mol
4) Aluminum sulfate : 342.3 g/mol
Al2(SO4)3
5) Ca(NO3)2 : 164.1 g/mol
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What is the mass of one mole of table salt (NaCl)?
a) 23.0 gb) 35.5 gc) 58.5 gd) 100.0 g
Atomic mass Na = 23.0 g/mol
Atomic mass Cl = 35.5 g/mol
Mass of one mole of NaCl = 23.0 + 35.5 = 58.5 g
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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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Molar Mass Example #1:
How many grams are in 7.20 moles of dinitrogen trioxide?
MW of N2O3 = 2N + 3O = 2(14.0) + 3(16.0) = 76.0 g/mol
1 mole = 76.0 g N2O3
Dinitrogen trioxide = N2O3
3232 ON g547
1.00mol
g0.76ON mol20.7
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Molar Mass Example #2:
Find the number of moles in 92.2 g of iron(III) oxide.
MW of Fe2O3 = 2Fe + 3O = 2(55.8) + 3(16.0) = 159.6 g/mol
1 mole = 159.6 g Fe2O3
Iron (III) oxide = Fe2O3
3232 OFe mol578.0
159.6g
mol00.1OFe g2.92
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Gram ↔ Mole Conversion Practice Problems:
1) How many grams are in 1.77 mol of diphosphorus pentachloride?
2) Find the number of moles in 107.5 g of iron(II) chlorate.
3) Find the number of grams in 3.32 mole of KNO3.
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1) How many grams are in 9.45 mol of diphosphorus pentachloride?
P2Cl5 = 239.5 g/mol
5252
ClP g22601.00mol
g5.239ClP mol45.9
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2) Find the number of moles in 107.5 g of iron(II) chlorate.
Fe(ClO3)2 = 222.8 g/mol
2323
)Fe(ClO 482.0g 222.8
mol 1.00)Fe(ClO g5.107mol
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3) Find the number of grams in 3.32 mole of KNO3.
KNO3 = 101.1 g/mol
33
KNO g3361.00mol
g1.101OKN mol32.3
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What is the mass of 3.7 moles of NaCl?
a) 15.8 gb) 58.5 gc) 216.5 gd) 6.02 x 1023 g
gmol
gmol5.216
NaCl 5.58
1
NaCl 7.3
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What is the mass of one mole of water (H2O)?
a) 3.0 gb) 16.0 gc) 17.0 gd) 18.0 g
Atomic mass H = 1.0 g/mol
Atomic mass O = 16.0 g/mol
Mass of one mole of H2O = 2(1.0) + 16.0 = 18.0 g
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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
molg
molg44.8
OH 0.18
1
1
OH 152
2
2
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Holy Moley – I’m glad that is over!