Transcript 1 The Mole 6.02 X 10 23 2

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The Mole
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6.02 X 10
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Average atomic Masses
• Atomic masses on the Periodic Table are not
whole numbers since they are weighted averages
of Mass Numbers (P+N)
• Average atomic mass depends on two factorsmass and relative abundance of each isotope.
• Example- Cu-63 (69.17% and 62.94amu) and Cu65(30.83% and 64.93amu)
- Average atomic mass=
(69.17x62.94)+(30.83x64.93) divided by
100=63.55amu
- Do Practice Q1-2, p133.
STOICHIOMETRY
- the study of the
quantitative
aspects of
chemical
reactions.
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Launch lab p 319- How much is a
mole?
• Decades or dozens are counting units. The Mole is
also a counting unit.
• Measure a small item (paperclip, eraser, penny) in
cm using a ruler.
• If a mole is 6.02 X1023 items, how far will a mole
of your items, placed end-to-end lengthwise,
extend into space? Express your answer in meters.
• Convert this answer into light years (ly).
• (1 ly=9.46 X1015 m).
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How much is a mole?
• Compare the distance you calculated with
these astronomical distances:
• Distance to the nearest star (other than the
sun)=4.3 ly
• Distance to the center of the galaxy= 30,000
ly
• Distance to the nearest galaxy=2X106 ly
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The Mole
• A counting unit
• Similar to a dozen or gross, except
instead of 12, it’s 602 billion trillion
602,000,000,000,000,000,000,000
• 6.02 X 1023 (in scientific notation)
• This number (termed Avogadro’s
number) is named in honor of Amedeo
Avogadro (1776 – 1856), who studied
quantities of gases and discovered that
no matter what the gas was, there were
the same number of molecules present
Just How Big is a Mole?
• Enough soft drink cans to cover the
surface of the earth to a depth of
over 200 miles.
• If you had Avogadro's number of
unpopped popcorn kernels, and
spread them across the United
States of America, the 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.
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The Mole
･Atoms and molecules are extremely
small making it very difficult to measure
their masses individually. ﾐIt is easier to
weigh a large collection of these.
･A mole (abbreviated as mol) is defined
as the number of C atoms in exactly 12
grams of pure C-12.
･This number is called Avogadro’s
number.
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A Mole of Particles
Contains 6.02 x 1023 particles
1 mole C
= 6.02 x 1023 C atoms
1 mole H2O = 6.02 x 1023 H2O molecules
1 mole NaCl = 6.02 x 1023 NaCl “molecules”
(technically, ionics are compounds not
molecules so they are called formula units)
6.02 x 1023 Na+ ions and
6.02 x 1023 Cl– ions
Avogadro’s Number as
Conversion Factor
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6.02 x 1023 particles
1 mole
or
1 mole
6.02 x 1023 particles
Note that a particle could be an atom OR a molecule!
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Learning Check
1. Number of atoms in 0.500 mole of Al
a) 500 Al atoms
b) 6.02 x 1023 Al atoms
c) 3.01 x 1023 Al atoms
2.Number of moles of S in 1.8 x 1024 S atoms
a) 1.0 mole S atoms
b) 3.0 mole S atoms
c) 1.1 x 1048 mole S atoms
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Molar Mass
･The mass in grams of one mole of atoms of any
pure substance is known as its molar mass. The
unit used is g/mol (gmol-1).
･Molar mass of sodium (Na) = mass of exactly one
mole of Na atoms = 22.99 g/mol = mass of 6.022
x 1023atoms of Na.
･Molar mass of Uranium (U) = 238.03 g/mol.
･The atomic mass number of an element in a
periodic table = molar mass for the element
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Practice p 322
• Determine the number of Zn atoms in 2.5
mol of Zn.
• Calculate the number of molecules in 11.5
mol of water (H2O).
• How many molecules of AgNO3 are there in
3.25 mol of it?
• Calculate the number of oxygen atoms in 5
mol of oxygen molecules.
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Practice p 324
• How many moles contain each of the
following?
• 5.75 X 1024 atoms Al
• 2.50 X 1020 atoms Fe
• How many moles contain each of the
following molecules?
• 3.75 X 1024 CO2
• 3.58 X 1023 ZnCl2
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Practice p 328
• Determine the mass in grams of each of the
following
• 3.57 mol Al
• 42.6 mol Si
• Convert each given quantity in scientific notation to
mass in grams expressed in scientific notation
• 3.45 X 102 mol Co
• 2.45 X 10-2 mol Zn
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Practice p 329
• Determine the number of moles in each of
the following
• 25.5 g Ag
• 300 g S
• Convert each mass to moles. Express the
answer in scientific notation.
• 1.25 X 103 g Zn
• 1 kg Fe
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Learning Check!
Find the molar mass
(usually we round to the tenths place)
A. 1 mole of Br atoms =
B. 1 mole of Sn atoms =
79.9 g/mole
118.7 g/mole
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Molar Mass of Molecules and
Compounds
･1 mole of any compound = 6.022 x 1023units
of the compound.
･Molar masses of compounds are calculated by
adding the molar masses of the atoms present
in the compound.
･Calculate the molar mass of Ca3(PO4)2
--Need to look the molar masses of each of the
element present and multiply by the number of
the atoms present.
Learning Check!
A. Molar Mass of K2O = ? Grams/mole
B. Molar Mass of antacid Al(OH)3 = ?
Grams/mole
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Practice p 335 (bottom)
• Determine the molar mass of each
ionic compound• NaOH, CaCl2, KC2H3O2
• Calculate the molar mass of each
molecular compound- C2H5OH, HCN,
CCl4
• Sr(NO3)2, (NH4)3PO4, C12H22O11
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Practice p 335 (top)
• Determine the moles of Cl- ions in 2.5 moles of
ZnCl2.
• Calculate the number of moles of each element in
1.25 mol C6H12O6.
• Determine the number of moles of sulfate ions
present in 3 mol of Fe2(SO4)3.
• How many moles of oxygen atoms are present in 5
mol of P2O5?
• Calculate the number of moles of hydrogen atoms
in 1.15 X101 mol of water. Express the answer in
scientific notation.
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Learning Check
Prozac, C17H18F3NO, is a widely used
antidepressant that inhibits the uptake of
serotonin by the brain. Find its molar
mass.
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Calculations with Molar Mass
molar mass
Grams
Moles
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Converting Moles and Grams
Aluminum is often used for the structure
of light-weight bicycle frames. How
many grams of Al are in 3.00 moles of
Al?
3.00 moles Al
? g Al
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1. Molar mass of Al
1 mole Al = 27.0 g Al
2. Conversion factors for Al
27.0g Al
1 mol Al
or
1 mol Al
27.0 g Al
3. Setup 3.00 moles Al
Answer
x
27.0 g Al
1 mole Al
= 81.0 g Al
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Learning Check!
The artificial sweetener aspartame
(Nutra-Sweet) formula C14H18N2O5 is
used to sweeten diet foods, coffee and
soft drinks. How many moles of
aspartame are present in 225 g of
aspartame?
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Practice p 336
• What is the mass of 3.25 mol of H2SO4?
• What is the mass of 4.35 X 101 mol of
ZnCl2?
• Write the chemical formula for potassium
permanganate, and then calculate the mass
in grams of 2.55 mol of the compound.
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Practice p 337
• Determine the number of moles present in
each compound-22.6 g AgNO3, 6.5 g
ZnSO4, 35.0 g HCl.
• Identify each as an ionic and molecular
compound and convert the given mass to
moles. Express your answers in scientific
notation- 2.5 kg Fe2O3, 25.4 mg PbCl4.
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Atoms/Molecules and Grams
• Since 6.02 X 1023 particles = 1 mole
AND
1 mole = molar mass (grams)
• You can convert atoms/molecules to
moles and then moles to grams! (Two step
process)
• You can’t go directly from atoms to
grams!!!! You MUST go thru MOLES.
• That’s like asking 2 dozen cookies weigh
how many ounces if 1 cookie weighs 4 oz?
You have to convert to dozen first!
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Calculations
molar mass
Grams
Avogadro’s number
Moles
particles
Everything must go through
Moles!!!
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Atoms/Molecules and Grams
How many atoms of Cu are
present in 35.4 g of Cu?
35.4 g Cu
1 mol Cu
63.5 g Cu
6.02 X 1023 atoms Cu
1 mol Cu
= 3.4 X 1023 atoms Cu
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Learning Check!
How many atoms of K are present in
78.4 g of K?
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Learning Check!
What is the mass (in grams) of 1.20 X
1024 molecules of glucose (C6H12O6)?
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Learning Check!
How many atoms of O are present in
78.1 g of oxygen?
78.1 g O2 1 mol O2 6.02 X 1023 molecules O2 2 atoms O
32.0 g O2 1 mol O2
1 molecule O2
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Practice p 339
• A sample of ethanol C2H5OH has a mass of
45.6 g.- How many C atoms does the sample
contain? How many H atoms are present?
How many O atoms are present?
• A sample of Na2SO3 has a mass of 2.25 g.How many Na+ ions are present? How many
SO32-ions are present?What is the mass in
grams of one molecule of Na2SO3?
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Contd• A sample of CO2 has a mass of 52 g.- How many
C atoms are present? How many O atoms are
present? What is the mass in grams of 1 molecule
of CO2?
• A sample of silver chromate has a mass of 25.8 g.Write the formula for silver chromate. How many
cations are present? How many anions are present?
What is the mass in grams of 1 molecule of silver
chromate?
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Percent Composition of
Compounds
• Composition of compounds can be described
in 2 ways: By the number of its constituent
atoms. By the mass (%) of each element
present.
• ･The mass percents of elements are obtained
by comparing the mass of each element
present in 1 mole of the compound to the total
mass of the compound.
• ･Useful today with unknown compounds.
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Percent Composition
What is the percent carbon in C5H8NO4 (the
glutamic acid used to make MSG
monosodium glutamate), a compound used
to flavor foods and tenderize meats?
a) 8.22 %C
b) 24.3 %C
c) 41.1 %C
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Practice p 344
• What is the percent composition of H3PO4?
• Which has the larger percent by mass of
sulfur H2SO3 or H2S2O8?
• Calculate the percent by mass of each
element in CaCl2.
• Sodium sulfate is used in the manufacture of
detergents- Identify each of the elements of
sodium sulfate, and write the formula. identify the compound as ionic or covalentcalculate the percent by mass of each
element in sodium sulfate.
Chemical Formulas of Compounds
• Formulas give the relative numbers of atoms or
moles of each element in a formula unit - always a
whole number ratio (the law of definite
proportions).
NO2
2 atoms of O for every 1 atom of N
1 mole of NO2 : 2 moles of O atoms to every 1
mole of N atoms
• If we know or can determine the relative number
of moles of each element in a compound, we can
determine a formula for the compound.
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Types of Formulas
• Empirical Formula
The formula of a compound that
expresses the smallest whole number
ratio of the atoms present.
(Ionic formulae are always empirical
formulae)
• Molecular Formula
The formula that states the actual
number of each kind of atom found in one
molecule of the compound. Example- CH
is the empirical formula for benzene,
C6H6).
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• Molecular formula is a multiple of the
empirical formula. Sometimes EF is the
same as MF (multiple of one).
• To go from empirical formula to molecular
formula, you multiply by multiplication
factor!
• Empirical formula X multiplication factor
= molecular formula
To obtain an Empirical Formula
1. Determine the mass in grams of each
element present, if necessary.
2. Calculate the number of moles of each
element.
3. Divide each by the smallest number of
moles to obtain the simplest whole
number ratio.
4. If whole numbers are not obtained* in
step 3), multiply through by the smallest
number that will give all whole numbers
* Be
careful! Do not round off numbers prematurely
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Empirical Formulas- Calculation
steps•
•
•
•
Change Percent to mass, if needed.
Mass to mole (divide by Atomic Mass)
Divide by smallest
Multiply till whole
A sample of a brown gas, a major air pollutant,
is found to contain 2.34 g N and 5.34g O.
Determine a formula for this substance.
require mole ratios so convert grams to moles
moles of N = 2.34g of N = 0.167 moles of N
14.01 g/mole
moles of O = 5.34 g = 0.334 moles of O
16.00 g/mole
N 0.167 O 0.334  NO 2
Formula: N O
0.167
0.334
0.167
0.167
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Calculation of the Molecular Formula
A compound has an empirical formula
of NO2. The colourless liquid, used in
rocket engines has a molar mass of
92.0 g/mole. What is the molecular
formula of this substance?
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Empirical Formula from % Composition
A substance has the following composition by
mass: 60.80 % Na ; 28.60 % B ; 10.60 % H
What is the empirical formula of the substance?
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Practice p 346
• A compound has 63.16% O and 36.84%N.
What is the empirical formula of this
compound?
• Determine the empirical formula of a
compound containing 35.98% Al and
64.02%S.
• Propane contains 81.82% C and 18.18% H.
What is the empirical formula ?
• Aspirin has 60% C, 4.44% H, and 35.56%
O. Determine the empirical formula of this
compound.
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Practice p 350
• A compound has 49.98 g C and 10.47g H. It’s Molar
mass is 58.12g. Determine it’s molecular formula.
• A liquid has 46.68% N and 53.32% O, molar mass is
60.01g. What is the molecular formula?
• An oxide of potassium has 19.55g K and 4 g of O.
What is it’s empirical formula?
• A compound has 65.45 % C, 5.45%H and 29.09% O.
If the molar mass is 110g, what is its molecular
formula?
• Morphine has 17.9g C, 1.68g H, 4.225g O and 1.228
g N. Determine the empirical formula of morphine.
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Formulas of hydrates
• Hydrate is a compound with a fixed number
of water molecules bound to it.
• Na2CO3.10H2O- sodium carbonate
decahydrate
• Hydrate+ heat= anhydrous compound
(without water)
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How to find out the formula of a
hydrate
• Need to know how many moles of H20 attached to
the molecule- BaCl2.xH2O
• Mass sample
• Heat it, mass again.
• The difference in mass= mass of water
• Divide it by molar mass of H20 (18g)= moles of
water
• Determine moles of compound as well.
• Determine ratio of water molecules to compound
molecules.
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Try it!
• A mass of 2.5 g of blue, hydrated copper
sulfate (CuSO4.xH2O) is placed in a
crucible and heated. After heating, 1.59 g of
white anhydrous copper sulfate (CuSO4)
remains. What is the formula for the
hydrate?
Practice p 353
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• A hydrate has 48.8% MgSO4 and 51.2% H2O. What
is its formula and name?
• An 11.75 g sample of a common hydrate of cobalt
(II) chloride is heated. After heating, 0.0712 mol of
anhydrous cobalt chloride remains. What is the
formula and name of this hydrate?
• P354 q81- Arrange these hydrates in order of
increasing percent water content- MgSO4.7H2O,
Ba(OH)2.8H2O, CoCl2.6H2O
Hydrate review
• 1. A hydrate of magnesium sulfate has a
mass of 13.52 g. This sample is heated until
no water remains. The MgSO4 anhydrate has
a mass of 6.60 g. Find the formula and name
of the hydrate.
• 2. A sample of copper (II) sulfate hydrate
has a mass of 3.97 g. After heating, the
CuSO4 that remains has a mass of 2.54 g.
Determine the correct formula and name of
the hydrate.
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Empirical/molecular formula review
• Analysis of a certain compound yielded the
following percentages of the elements by
mass: N 29.16%, H 8.392%, C 12.5%, O
49.95%. Determine the empirical formula of
the compound.
• If 1.25 g of Al is heated in F2 gas, 3.89g of
aluminum fluoride results. Determine the
empirical formula for aluminum fluoride.
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