chapter 10 chemical quantities. a representative particle (rp) refers to the species present in a...
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![Page 1: Chapter 10 Chemical Quantities. A representative particle (RP) refers to the species present in a substance, usually atoms(S), molecules(SO 2 ), or formula](https://reader038.vdocuments.site/reader038/viewer/2022110209/56649e555503460f94b4d475/html5/thumbnails/1.jpg)
Chapter 10 Chemical Quantities
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A representative particle (RP) refers to the species present in a substance, usually atoms(S), molecules(SO2), or
formula units(NaCL)
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A representative particle (RP) refers to the species present in a
substance, usually
Element: atoms, Covalent Bond: molecules, or
Ionic Bond: formula units
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A representative particle (RP) is: 1 atom, 1 molecule,
or 1 formula unit.
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3 Word Summary:Representative Particle =
Atoms, Molecules or Ionic Formula
.
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How many atoms do you see?
Molecules?
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How many atoms do you see?
Molecules?
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How many atoms do you see?
Molecules?
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How many atoms do you see?
Molecules?
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You must state very specifically what the particle
represents: atoms or
molecules and of what?
State what is the RP: An atom of O, An atom of C or a molecule of CO2?
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Does this look like air? Does air
have a representative
particle?
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Answer is NO! There is not a
particle of air. Air is about 80% N2 and 20% O2.
Air is composed of several
representative particles mixed
together.
So Mixtures do NOT have representative particles.
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The mole = mol6.02 x 1023 representative
particles (RP) of a substance is called Avogadro's number.
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MEMORIZE:
Mole =
6.02 x 1023
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6.02 x 10 23
Emphasis is on 10 23
Why on the 23 and not the 6.02?
1.) If you have $5 x 10 5+/- $1 Does the 1 matter?
2.) If you have $5 x 10 5 +/- 10 1 Does it matter?
Which is more important?
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1.) If you have $5 x 105 +/- $1 Does the 1 matter?
This ranges from 400,000 to 600,000
2.) If you have $5 x 10 5 +/- 101 Does the 1 matter?
This ranges from $50,000 to $5 million.
Which is more important?1.) 400,000 to 600,000 or 2.) $50,000 to $5 million
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A mole is just a name of a number.
Like Pi = 3.14159265 and e = 2.718
Mole =
6.02 x 1023
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A mole is just a name of a number. Like Thousands, Millions, Billions, Trillions, Quadrillions, Gazillionbillions
Mole =
6.02 x 1023
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There is a very specific reason that we use a mole,
Atomic Mass in grams is equal to 1 mole of an element.
Do some examples Have students do elements off the periodic table.Shoe 1 mole samples on counter..
Molar Mass = grams of 1 mole of atoms = Atomic Mass
6.02 x 1023
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Avogadro discovered the mole, but the exact number was
determine later. So it was named after. So it’s 2nd name is
Avogadro's number
6.02 x 1023
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Review Dimensional Analysis.Known x Conversion Factor = Wanted
Known x Wanted = Wanted
KnownExample, convert feet to inches.
4 ft x 12 inches = 48 inches
1 ft .
1.) Do the dimensions or units first.
Cross off feet and inches are left.
2.) Fill in # and multiply and divide the numbers.
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How many atoms of sodium are in 2.0 moles?
Na = RP
Note: Adjust answer for 1.) Scientific Notation2.) Significant Figures
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How many carbon atoms are in 3.0 moles of C2S?
1 molecule C2S = 1 RP
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How many carbon atoms are in 3.0 moles of C2S?
1 molecule C2S = 1 RP1 RP has 2 C atoms
3 mol of C2S x 2 C atoms = 6 mol C
= 6 mol C x 6.0 x 1023 atoms/mol = 36 x 1023 atoms = 3.6 x 1024 atoms
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How many grams of carbon are in 3.0 moles of C2S?
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How many grams of carbon are in 3.0 moles of C2S?
3.0 mol C2S = 6.0 mol C
= 6.0 mol C x 12 g/mol C = 72g C
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How many pennies is 1 mole
of pennies?
Would it cover the earth?
How deep?
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How much is a mole of pennies? A mole of pennies would cover the
entire Earth to a depth of 300 m,
or 3 football fields (With end zones).
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Molar Road Map: Conversion Factors for moles. Pg 323
# of Atoms = moles x 6.0 x 1023 atoms/mol
Mass (g) =
moles x atomic mass (from periodic table)
Volume of Gas = (at STP)
moles x 22.4 L / mol
STP = Standard Temperature and Pressure = 0° C, 101.3 kPa
= 1 atmospheric pressure at sea level on a freezing day.
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Nest section uses:Molar Road Equations
# of Atoms =
moles x 6.0 x 1023 atoms/mol
Mass (g) =
moles x atomic mass (from periodic table)
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How many hydrogen atoms are in 1.5 moles of hydrogen?
•
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How many hydrogen atoms are in 1.5 moles of hydrogen?
1 atom H = 1 RP1 RP has 1 H atom
1.5 mol of H x 1 H atom = 1.5 mol H
1.5 mol H x 6.0 x 1023 atoms/mol = 9.0 x 1023 atoms
Always ask, is Sci Not and Sig Figs correct?
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How many hydrogen atoms are in 1.5 moles of hydrogen?
Part 2: What is their mass?
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How many hydrogen atoms are in 1.5 moles of hydrogen?
Part 2: What is their mass? 1 atom H = 1 RP
1 RP has 1 H atom
1.5 mol of H x 1 H atom = 1.5 mol H
Mass = moles x atomic mass
1.5 mol H x 1.0 g/mol
= 1.5 g H
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How many hydrogen atoms are in 1.5 moles of water?
•
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How many hydrogen atoms are in 1.5 moles of water?
1 molecule H2O = 1 RP1 RP has 2 H atoms
1.5 mol of H2O x 2 H atom / mol= 3.0 mol H
3.0 mol H x 6.02 x 1023 atoms/mol = 18.06 x 1023 atoms
= 1.8 x 1024 atoms
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How many grams of hydrogen are in 1.5 moles of water?
•
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How many grams of hydrogen are in 1.5 moles of water?
1 molecule H2O = 1 RP1 RP has 2 H atoms
1.5 mol of H2O x 2 H atom / mol= 3.0 mol H
Mass = moles x atomic mass
3.0 mol H x 1.0 g/mol
= 3.0 g H
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How many moles of carbon are in 1.0 mole of C2S dicarbon
monosulfide?• A) 1 mole
• B) 2 moles
• C) 3 moles
• D) 4 moles
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How many moles of carbon are in 1.0 mole of C2S dicarbon
monosulfide?• A) 1 mole
• B) 2 moles
• C) 3 moles
• D) 4 moles
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What is the molar mass of 1 mol of calcium?
• 1 mole of any element is that compounds atomic mass expressed in grams
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What is the molar mass of 1 mol of calcium?
• 1 mole of any element is that compounds atomic mass expressed in grams
• 1 mole Ca = 40.8 g / mol
• Because atomic mass is 40.8 amu
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What is the molar mass of calcium hydroxide?
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What is the molar mass of calcium hydroxide?
Ca(OH)2
List each atom and it’s quantity. Multiply by it’s atomic mass
add.Ca x 1 O x 2 H x 2 40 x 1 16 x 2 1 x 2
40 x 1 + 16 x 2 + 1 x 2 = = 74g
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Common Atomic MassesH 1
C 12N 14O 16Ne 20 Fe 56 U 238
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What is the molar mass of the following?
• Neon
• Dinitrogen monoxide
• Calcium chloride
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Ne = 20gN2O=44g
CaCl2 = 110g
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What is the molar mass of Mg(C2H3O2)2?
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What is the molar mass of Mg(C2H3O2)2? 142g
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• How many moles are in 55g of carbon?
• How many grams are in 22 moles of CO2?
• How many moles in 55g Ne? • How many moles in 55g oxygen?
• How many C atoms in 55g C4H10?
• How many H atoms in 155g HC2H3O2? • Answers on Following Slides
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How many moles are in 55g of carbon?
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How many grams are in 22 moles of CO2?
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How many moles in 55g Ne?
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How many moles in 55g oxygen?
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How many C atoms in 55g C4H10?
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How many H atoms in 155g HC2H3O2?
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GAS VOLUME
1 mole of any gas at STP is
22.4L
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MEMORIZE1 mole of any gas at STP is
22.4LRemember this WOD?
Volume of Gas = (at STP) moles x 22.4 L / mol
STP = Standard Temperature and Pressure = 0° C, 101.3 kPa
See mole box on page 301.
• What does STP stand for?
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1 mole of any gas at STP is 22.4L.
• What does STP stand for?
• Standard temperature and pressure
• 0oC and 1 atm
• Where is it 1 atm?
• Why pick 0oC?
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1 mole of any gas at STP is 22.4L.
• What does STP stand for?
• Standard temperature and pressure
• 0oC and 1 atm
• Where is it 1 atm? ANS: Sea Level
• Why pick 0oC? ANS: Freezing temp is easy to recreate.
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How many atoms are in 44.8L of oxygen?
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How many C atoms are in 2.2L of C3H8(g)?
• (g) at the end means it is a gas.
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How many L are in 3.4 x 1023 CO2 molecules?
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How many carbon monoxide moles are in 44.8L of CO?
• A) 1 mol
• B) 2 mol
• C) 1.00 mol
• D) 2.00 mol
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Similar Test Question• One drop of H2O has a mass of 0.1g. How
many atoms of hydrogen are contained in a single drop of water?
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Start 10.3
Percent composition
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Percent composition = % of elements that make a compound
mass (element) ÷ mass (compound) x 100% =
Percent is about mass,
not volume, not moles, not atoms or molecules.
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What is the percent composition of H2O?
• Use molar masses.• mass (element) ÷ mass (compound) x 100% =
» % Composition
• Hydrogen H / Total x 100%• 2g/18g x 100% = 11.1% Hydrogen• Oxygen O / Total x 100%• 16g/18g x 100% = 88.9% Oxygen• Total = 100% (or close because of rounding)
• 11.1% H and 88.9% Oxygen = 100%
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What is the percent composition of carbon tetrafluoride?
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Which has a higher percentage of carbon CO or C3H8OH?
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Element Mass = Percent composition x Total Mass
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A 175g sample of CO2 contains how many g of carbon?
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Similar Test Question• How many grams of sodium can be
obtained from 42.5g of sodium nitrate?
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Empirical formula = lowest ratio of elements in a compound, same %
composition
• C2H4 C4H8
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Which of the following is an example of an empirical
formula?• A) CO
• B) C2H2
• C) C2Cl4
• D) C2H6
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Test (like) Question
• The compound is 5.9% H. What is the molecular formula and empirical formula for this compound if it is only composed of oxygen and hydrogen?
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Solution• 100% = 100g• 5.9%H = 5.9gH 94.1%O = 94.1gO
• Convert grams to moles• 5.9 mol H 5.9 mol O
• Divided by smallest to find EF (emp. Form.)• (5.9/5.9) 1mol H 1 mol O• 1g + 16g = 17g
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Solution
• Multiply to find MF (molecular formula)
• OH(17g) x 2 = 34
• H2O2
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Test (like) question
• 20.0g of sugar will produce how much carbon?
• Sugar = C12H22O11
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Solution
• Find percent composition of Carbon
• 144g C / 342g C12H22O11 x 100%
• 42.1% C
• Find amount of carbon (decimal not %)
• 0.421 x 20g = 8.42g C
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• 20.0g powdered sugar (C12H22O11) to 10 ml 18M sulfuric acid.
• Carbon and steam (water) will be produced.
• Add water/sodium bicarbonate to clean.
• Solid in trash.
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Review Molar Mass
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Gram atomic mass – atomic mass of 1 mol of an element
expressed in grams1 mol carbon = 12g
Gram molecular mass – mass of 1 mol of that compound
1 mole H2O = 18g
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Gram formula mass – mass of 1 mol of an ionic compound
1 mol of NaCl = 58 g
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Molar mass – the mass of 1 mole of any element or compound
(add atomic masses)
1 mol of NaCl = 58 g/mol23+35
1 mol carbon = 12g/mol12
1 mole H2O = 18g/mol 1+1+16