Quantitative aspects of chemical change - WordPress.com · 8/3/2018 · Quantitative aspects of...
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Quantitative aspects of chemical change
sdfgsfgfgsgf
Grade 10 Physical Science
CAPS
2016
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The mole concept
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The mole concept
• Atoms are small – chemists know this.
• But somewhere along the line – they have to count them.
• The mole is the SI Unit for the measurement of the amount
of matter.
• A mole is a large group of atoms or molecules, which can
be described as a specific amount of matter, or the
number of particles.
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The mole concept
• The particles of an element is called “atoms.”
• The particles of a covalent compound is called
“molecules.”
• The particles of an ionic compound is called “ions.”
“Particles”
NaNa
Na
Na
H
H
OH
HO𝐻2𝑂
𝑁𝑎𝐶𝑙
NaCl
Na
Cl
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The mole concept
• A mole is that quantity of matter that has the
• same number of particles as there are in 12g of carbon
12.
• How much is this “number of particles?”
• Avogardo’s number
Who is Avogardo?
Some clever Italian scientist….
What is this number?
6.02 × 1023
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The mole concept
•How big is that?
• It’s 602 000 000 000 000 000 000 000
•That’s nice….how BIG IS THAT?!
Go and read on page 196
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The mole concept
• This means that…
• 1 mole of a substance contains 6.02 × 1023 units
• Example:
• 1 mole of sodium means 6.02 × 1023 sodium atoms
• 1 mole of 𝐻2𝑂 means 6.02 × 1023 𝐻2𝑂 molecules.
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The mole concept
• So just like:
• A dozen = 12
• A pair = 2
• A case = 24
• SO a Mole = 6.02 × 1023
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The mole concept
• So if I could put all of these
particles onto a scale – what
would it’s mass be?
• The mass of 1 mole of a substance is equal to it’s atomic
mass in grams.
• 1 mole Na = 23g
• 1 mole Mg = g
• 1 mole 𝑂2 = g2432
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The mole concept
• So if I could put all of these
particles onto a scale – what
would it’s mass be?
• The mass of 1 mole of a substance is equal to it’s atomic
mass in grams.
• 1 mole 𝑀𝑔𝑂 = g
• 1 mole 𝑁𝑎𝑂𝐻 = g
• 1 mole 𝐻2𝑆𝑂4 = g
244098
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The mole concept
Molecular Mass
• Since particles are so small, it’s difficult to use g or kg to
calculate their masses.
• Hence we used the atomic mass unit (u)
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The mole concept
There’s a difference
• Symbol: M
• Unit: 𝑔.𝑚𝑜𝑙−1
• Used for an
element• Eg.𝑀 𝐶𝑢 = 63.53𝑔.𝑚𝑜𝑙−1
• 𝑀 𝑀𝑔 =• M 𝐶𝑎 =
Atomic mass Molar mass Formula mass
• Symbol: 𝑀• Unit: 𝑔.𝑚𝑜𝑙−1
• Used for an ionic
compound.• Eg.𝑀 𝑁𝑎𝐶𝑙 = 58.5𝑔.𝑚𝑜𝑙−1
• 𝐴𝑟 𝑀𝑔𝑆𝑂4 =• 𝐴𝑟 𝐾𝑂𝐻 =
• Symbol: M
• Unit: 𝑔.𝑚𝑜𝑙−1
• Used for an
compound• Eg.𝑀 𝐻2𝑂 = 18𝑔.𝑚𝑜𝑙−1
• 𝑀 𝐻𝐶𝑙 =• 𝑀 𝐶𝑂2 =
24𝑔.𝑚𝑜𝑙−1
40𝑔.𝑚𝑜𝑙−136.5𝑔.𝑚𝑜𝑙−1
44𝑔.𝑚𝑜𝑙−1
120𝑔.𝑚𝑜𝑙−1
56𝑔.𝑚𝑜𝑙−1
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The mole concept
There’s a difference
• Symbol: 𝐴𝑟• No unit
• Used for an
element• Eg.𝐴𝑟 𝐶𝑢 = 63.53• 𝐴𝑟 𝑀𝑔 =• 𝐴𝑟 𝐶𝑎 =
Relative Atomic mass
Relative Molar mass
Relative Formula mass
• Symbol:𝑀𝑟
• No unit
• Used for an ionic
compound.• Eg.𝑀𝑟 𝑁𝑎𝐶𝑙 = 58.5• 𝑀𝑟 𝑀𝑔𝑆𝑂4 =• 𝑀𝑟 𝐾𝑂𝐻 =
• Symbol: 𝑀𝑟
• No unit
• Used for a
compound.• Eg.𝑀𝑟 𝐻2𝑂 = 18• 𝑀𝑟 𝐻𝐶𝑙 =• 𝑀𝑟 𝐶𝑂2 =
2440
36.544
12056
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The mole concept
Let’s practice…
Substance Number of moles
Mass in grams
Particles Number of particles
Carbon 1 12 Atoms 6.02 × 1023
1
1
1
Cobalt Atoms 𝟔. 𝟎𝟐 × 𝟏𝟎𝟐𝟑59
Carbon dioxide
molecules
𝟔. 𝟎𝟐 × 𝟏𝟎𝟐𝟑44
Sodium Chloride
ions 𝟐 × 𝟔. 𝟎𝟐 × 𝟏𝟎𝟐𝟑58.5
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homeworkExercise 20 pg. 198-199
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The relationship between:
mole mass molar mass
n m M( ) (g) (g.mol-1)
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𝑛 =𝑚
𝑀
mol
mass
Molar mass
( )
(𝒈)
(𝒈.𝒎𝒐𝒍−𝟏)
TB. PG 229
The equation #1
Relationship between mole, mass and molar mass
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𝑛 =𝑛𝑜. 𝑜𝑓 𝑝𝑎𝑟𝑡𝑖𝑐𝑙𝑒𝑠
𝑁𝐴
mol
Avogardo’s number:
𝟔. 𝟎𝟐 × 𝟏𝟎𝟐𝟑
( )
TB. PG 229
The equation #2
Relationship between mole, mass and molar mass
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worksheet
Relationship between mole, mass and molar mass
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Empirical formulaThis is the simplest ratio in which the elements of the
compound bonds with each other.
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𝐻2𝑂
This formula says that 1 water molecule has:
• 2 hydrogen atoms and 1 oxygen atom.
• 1 mole 𝐻2𝑂 contains 6.02 × 1023 water molecules
• So that means there are 2 × 6.02 × 1023hydrogen atoms and 1 × 6.02 × 1023 oxygen atoms.
OH
H
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worksheet
Empirical formula
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HomeworkExercise 21 pg. 202-203
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Percentage Composition
Used to determine the composition of a substance according
to a percentage division.
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Example 1
Determine the percentage composition of 𝑁𝑎𝐻𝐶𝑂3.
Step 1
Find the formula mass of 𝑁𝑎𝐻𝐶𝑂3. 84𝑔.𝑚𝑜𝑙−1
Step 2Find the atomic mass of each element in the
compound.
𝑀 𝑁𝑎= 23𝑔.𝑚𝑜𝑙−1
𝑀 𝐻= 1𝑔.𝑚𝑜𝑙−1
𝑀 𝐶= 12𝑔.𝑚𝑜𝑙−1
𝑀 𝑂= 16𝑔.𝑚𝑜
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Step 3
Calculate!!!!
𝑚𝑎𝑠𝑠 𝑜𝑓 𝑒𝑙𝑒𝑚𝑒𝑛𝑡 (𝑔.𝑚𝑜𝑙−1)
𝑓𝑜𝑟𝑚𝑢𝑙𝑎 𝑚𝑎𝑠𝑠 (𝑔.𝑚𝑜𝑙−1)× 100 =
𝑁𝑎 = 27.38% 𝐻 = 1.19% 𝐶 = 14.29%
𝑂 = 57.14%
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Homework EXERCISE 22 PG. 205-206
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Step 1
Find the formula mass of 𝑁𝑎𝐻𝐶𝑂3.
Step 2Find the atomic mass of each element in the compound.
Step 3
𝑚𝑎𝑠𝑠 𝑜𝑓 𝑒𝑙𝑒𝑚𝑒𝑛𝑡 (𝑔.𝑚𝑜𝑙−1)
𝑓𝑜𝑟𝑚𝑢𝑙𝑎 𝑚𝑎𝑠𝑠 (𝑔.𝑚𝑜𝑙−1)× 100 =
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Compound Composition
Used to determine the amount of mol water from
crystallization.
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Example 1
Weigh out 2.5g of 𝐶𝑢𝑆𝑂4. 𝑛𝐻2𝑂 crystals.
Dry the crystals by heating them gently in a crucible. This is done to remove the water.
Weigh the crystals again.
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Example 1
At start: 2.5g of 𝐶𝑢𝑆𝑂4. 𝑛𝐻2𝑂
After drying: 1.6g of 𝐶𝑢𝑆𝑂4
So, in 2.5g of 𝐶𝑢𝑆𝑂4. 𝑛𝐻2𝑂
1.6g was 𝐶𝑢𝑆𝑂4 0.9g was 𝑯𝟐𝑶and
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Example 1
Just like Empirical Formula
𝑛𝐶𝑢𝑆𝑂4 =𝑚
𝑀=
1.6
159.5= 0.01𝑚𝑜𝑙
𝑛𝐻2𝑂 =𝑚
𝑀=0.9
18= 0.05𝑚𝑜𝑙
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Example 1
Ratio
𝐶𝑢𝑆𝑂4: 𝐻2𝑂
0.01: 0.05
1: 5
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Example 1
SO!!!! 1 𝐶𝑢𝑆𝑂4. 5𝐻2𝑂 crystals.
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Example 2
Weigh out 6.25g of 𝑀𝑔𝑆𝑂4. 𝑛𝐻2𝑂 crystals.
Dry the crystals by heating them gently in a crucible. This is done to remove the water.
Weigh the crystals again.
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Example 2
At start: 6.25g of 𝑀𝑔𝑆𝑂4. 𝑛𝐻2𝑂
After drying: 4g of 𝑀𝑔𝑆𝑂4
So, in 6.25g of 𝑀𝑔𝑆𝑂4. 𝑛𝐻2𝑂
4g was 𝑀𝑔𝑆𝑂4 2.25g was 𝑯𝟐𝑶and
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Example 1
Just like Empirical Formula
𝑛𝑀𝑔𝑆𝑂4 =𝑚
𝑀=
4
120= 0.03𝑚𝑜𝑙
𝑛𝐻2𝑂 =𝑚
𝑀=2.25
18= 0.13𝑚𝑜𝑙
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Example 2
Ratio
𝑀𝑔𝑆𝑂4 ∶ 𝐻2𝑂
0.03: 0.13
1: 4
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Example 2
SO!!!! 1 𝑀𝑔𝑆𝑂4. 4𝐻2𝑂 crystals.
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Determine the number of moles of water of
crystallization in 5.4g of 𝐴𝑙𝐶𝑙3. 𝑛𝐻2𝑂.
Workbook Exercise
Write down and complete the following
example in your workbook.
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Molar gas volume
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1 mole of a gas occupies a volume of 22.4 𝑑𝑚3 at STP.
𝑶𝟐
𝑶𝟐𝑶𝟐
𝑶𝟐
𝑶𝟐
𝑶𝟐
𝟐𝟐. 𝟒𝒅𝒎𝟑
•What is STP???
Standard temperature
and pressure𝑜℃ 𝑜𝑟 273𝐾
101.3𝑘𝑃𝑎
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𝑛 =𝑉
𝑉𝑚
mol
volume
Molar gas volume
( )
(𝒅𝒎𝟑)
(𝟐𝟐. 𝟒𝒅𝒎𝟑)
TB. PG 229
The equation # 1
Molar gas volume
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𝑛 =𝑚
𝑀
mol
mass
Molar mass
( )
(𝒈)
(𝒈.𝒎𝒐𝒍−𝟏)
TB. PG 229
The equation #2
Molar gas volume
![Page 45: Quantitative aspects of chemical change - WordPress.com · 8/3/2018 · Quantitative aspects of chemical change sdfgsfgfgsgf Grade 10 Physical Science CAPS 2016. The mole concept.](https://reader035.fdocuments.us/reader035/viewer/2022071003/5fc089a653cc495a364ba608/html5/thumbnails/45.jpg)
𝑛 =𝑛𝑜. 𝑜𝑓 𝑝𝑎𝑟𝑡𝑖𝑐𝑙𝑒𝑠
𝑁𝐴
mol
Avogardo’s number:
𝟔. 𝟎𝟐 × 𝟏𝟎𝟐𝟑
( )
TB. PG 229
The equation #3
Molar gas volume
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•Calculate the mass of 5.6𝑑𝑚3 of 𝐶𝑂2 at STP.
Example 1
What are you given?
What do you want to find?
![Page 47: Quantitative aspects of chemical change - WordPress.com · 8/3/2018 · Quantitative aspects of chemical change sdfgsfgfgsgf Grade 10 Physical Science CAPS 2016. The mole concept.](https://reader035.fdocuments.us/reader035/viewer/2022071003/5fc089a653cc495a364ba608/html5/thumbnails/47.jpg)
Homework EXERCISE 23 pg. 207-209
1.1
2.1
3.15.1
4.1
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ConcentrationThis is the quantity of a dissolved solute in mole per 𝑑𝑚3 of
solution.
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𝑐 =𝑛
𝑉
mol
Volume
(𝒎𝒐𝒍. 𝒅𝒎−𝟑)
( )
(𝒅𝒎𝟑)
USE IF YOU ARE GIVEN
MOLE
The equation # 1
Concentration
concentration
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𝑐 =𝑚
𝑀𝑉
mass
Volume
(𝒎𝒐𝒍. 𝒅𝒎−𝟑)
( 𝒈 )
(𝒅𝒎𝟑)
USE IF YOU ARE GIVEN
MASS
The equation # 1
Concentration
concentration
Molar mass
(𝒈.𝒎𝒐𝒍−𝟏)
![Page 51: Quantitative aspects of chemical change - WordPress.com · 8/3/2018 · Quantitative aspects of chemical change sdfgsfgfgsgf Grade 10 Physical Science CAPS 2016. The mole concept.](https://reader035.fdocuments.us/reader035/viewer/2022071003/5fc089a653cc495a364ba608/html5/thumbnails/51.jpg)
Oh! But converting is so VERY vital
𝑚𝑚3 𝑐𝑚3 𝑑𝑚3 𝑚3
× 1000× 1000× 1000
÷ 1000 ÷ 1000 ÷ 1000
![Page 52: Quantitative aspects of chemical change - WordPress.com · 8/3/2018 · Quantitative aspects of chemical change sdfgsfgfgsgf Grade 10 Physical Science CAPS 2016. The mole concept.](https://reader035.fdocuments.us/reader035/viewer/2022071003/5fc089a653cc495a364ba608/html5/thumbnails/52.jpg)
AND…
1c𝑚3 = 1𝑚𝑙1d𝑚3 = 1 𝑙𝑖𝑡𝑟𝑒
![Page 53: Quantitative aspects of chemical change - WordPress.com · 8/3/2018 · Quantitative aspects of chemical change sdfgsfgfgsgf Grade 10 Physical Science CAPS 2016. The mole concept.](https://reader035.fdocuments.us/reader035/viewer/2022071003/5fc089a653cc495a364ba608/html5/thumbnails/53.jpg)
•Calculate the concentration of a solution that contains 0.2 mol copper
(II) sulphate in 250𝑐𝑚3 water.
Example 1
What are you given?
What do you want to find?
![Page 54: Quantitative aspects of chemical change - WordPress.com · 8/3/2018 · Quantitative aspects of chemical change sdfgsfgfgsgf Grade 10 Physical Science CAPS 2016. The mole concept.](https://reader035.fdocuments.us/reader035/viewer/2022071003/5fc089a653cc495a364ba608/html5/thumbnails/54.jpg)
Homework EXERCISE 24 pg. 211-212
2.1
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Stoichiometric calculations
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•A chemical reaction occurs when substances
(reactants) react chemically and produce
new substances (products).
•We represent such a reaction with a
chemical formula.
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2𝐻2 + 𝑂2 → 2𝐻2𝑂
• 2 mole hydrogen reacts with 1 mole of oxygen to form 2 moles of water.
• 4 hydrogen atoms react with 2 oxygen atoms to form 2 water molecules.
• 2 hydrogen molecules react with 1 oxygen molecule to form 2 water molecules.
• 4g of 𝑯𝟐 reacts with 32g of 𝑶𝟐 to form 36g of 𝑯𝟐𝑶
+ →
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𝐶 + 𝑂2 → 𝐶𝑂2
• 1 mole carbon reacts with 1 mole of oxygen to form 1 mole of carbon dioxide.
• 1 carbon atom react with 2 oxygen atoms to form 1 carbon dioxide molecule..
• 12g of 𝑪 reacts with 32g of 𝑶𝟐 to form 44g of 𝑪𝑶𝟐
+ →
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Calculations
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Example 1 – mass-mass calculation
•Calculate the mass of oxygen obtained when 14.7g
of potassium chlorate decomposes completely to
form potassium chloride.
![Page 61: Quantitative aspects of chemical change - WordPress.com · 8/3/2018 · Quantitative aspects of chemical change sdfgsfgfgsgf Grade 10 Physical Science CAPS 2016. The mole concept.](https://reader035.fdocuments.us/reader035/viewer/2022071003/5fc089a653cc495a364ba608/html5/thumbnails/61.jpg)
Example 2 – mass-volume calculation
•What mass of potassium chlorate must be heated to
release 90𝒅𝒎−𝟑 of oxygen at STP?
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HOMEWORK
EXERCISE 25 PG. 215-217