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Transcript of t4. Bab 5-Tenaga Dan Perubahan Kimia
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Chapter 5
Energy and Chemical Changes
Tingkatan PCKBy
CHE AHAMAD BIN DAUD
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5.1 Understanding physical and chemical changes
Student will be able to :
explain what physical change is,explain what chemical change is,
give examples of physical changes in daily life,
give examples of chemical changes in daily life,Compare and contrast physical changes and
chemical changes.
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ENERGY CHANGES
CHEMICAL CHANGES PHYSICAL CHANGES
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EXAMPLE 1 REVIEW 1
EXAMPLE 2
REVIEW 2
EXAMPLE 3
REVIEW 3
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ENERGY CHANGES
EXOTHERMICREACTION
CHEMICAL CHANGES
ENDOTHERMICREACTION
PHYSICAL CHANGES
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Chemical Change Physical change
Similarities
Substances can undergo changes ..............................
Differences
New substances formed
Change in chemical composition
Reversibility
Energy needed
SIMILARITIES AND DIFFERENCES BETWEEN CHEMICALS
AND PHYSICAL CHANGES
physica l ly
Less
Yes
Yes
More
No
Easy
No
Dif f icul t
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THE END…
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A physical change is a change whichdoes not produce a new substance. Only the
physical state of the substance has
changed.
BACK
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A chemical change is a changewhich produces a new substance. The new
substance has chemical properties and
composition different from the originalsubstance.
BACK
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Iodine crystal
Ice cube
Iodine crystal
is heated, it
changes fromsolid to gas
Watch glass
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Iodine crystalpurple vapour(Iodine vapour)
Ice cube
Watch glass
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Iodine crystal
Ice cube
Watch glass
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Iodine crystal
Ice cube
Watch glass
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Iodine crystal
purple vapour(Iodine vapour)
Ice cube
Watch glass
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Iodine crystal
Ice cube
Watch glass
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Iodine crystal
Ice cube
Watch glass
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Iodine crystal
Ice cube
Watch glass
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Iodine crystal
purple vapour(Iodine vapour)
Ice cube
Watch glass
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Iodine crystal
Black crystal
Ice cube
Watch glass
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Iodine crystal
Black crystal
Ice cube
Watch glass
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Black crystal
Ice cube
Watch glass
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Black crystal
Ice cube
Watch glass
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Black crystal
Ice cube
Watch glass
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Black crystal
(iodine)Iodine vapour
Ice cube
Watch glass
BACK
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• When the ………….. is heated, purple …………
is formed.
• Iodine changes from ………….to ……… without
going through the ……….. state (sublimation).
• When the iodine vapour…………… the cold
………….. of the watch glass, the vapour changesback into ……….. state (black crystal).
• Solid ……………. forms on the lower surface
of the watch glass.
• The change of solid iodine into iodine vapour is
……………..
• This is a ………….change.
iodine vapour
solid gasliquid
touches
surface solid
iodine
reversible
physicalBACK
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ICE CUBE
BACK
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Water and ................ have the ...................... particles.
The differences between water and ice are in terms of the
...............................and ......................... of the particles.
Ice can easily ................... into .................. when it is
.......................
Is this a reversible process ? ........................
Is energy absorbed or released ? ...........................
Is new product formed ? .....................
ice same
arrangement movement
change
Absorbed
heated
water
Yes
No
BACK
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The magnesium .................... burns with a ............... flame and
forms .............. ash.
During the process:- ..................... and .................... are given off.
- Magnesium combines with ...................in the air to
form ………......................
- .................................. is different from
..................................,
Is this a reversible process ?........................
Is energy absorbed or released ? ...........................
Is new product formed ? .....................
r ibbon
heat
whi te
br ight
l ight
oxygen
magnes ium oxide
magnes ium oxide
magnes ium
magnes ium oxide
No
Yes
Magnesium + oxygen ………………………. (white ash )
(grey metal)
Released
BACK
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Iron nails ........................... when ........................ and .........................
are present.
Rusts is a ................. substance that consists of................................
Is this reversible process ? .....................
Is energy absorbed or released ? ...........................
Is new product formed ?.....................
................... + Oxygen + .................... ............................. (Rust)
rust oxyg en water
b rown iron oxide
Iron Water Iron ox ide
No
Absorbed
Yes
BACK
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An endothermic reaction is a reaction
which absorbs heat energy from the
surroundings.
BACK
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An exothermic reaction is a reaction which
releases heat energy to the surroundings.
BACK
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5.2 Analysing heat change in chemical reactions
Student will be able to :
State that chemical reactions involve heat change,
Identify reactions involving heat lost,Identify reactions involving heat gain,
Relate changes in temperature of reactants toexothermic reactions,
Relate changes in temperature of reactants toendothermic reactions,
Explain through examples heat changes that occurduring industrial chemical reaction.
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You are given ammonium chloride and sodium hydroxide as the
chemical substances.
Heat is absorbed or released during a chemical reaction
a. Based on the above statement, write a suitable hypothesis.
(1 mark)
b. Describe an experiment that you can carry out in the laboratory toprove this hypothesis.
Your description should contain the following:
i. Aim of the experiment (1 mark)
ii. Identify the variables (2 marks)
iii. List of apparatus and materials (1 mark)
iv. Method (4 marks)
v. Tabulation of data (1 mark) 39
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STATEMENT
WHAT I WANT TO CHANGE
MVWHAT IS FIXED
CVWHAT I SHOULD MEASURE
RV
WHEN I CHANGE, WHAT WILL HAPPEN TO WHAT I MEASURE (HYPOTHESIS)
WHY I DO … (AIM) To study ………………..
METHOD I USE ………………
PRO EDURE
DATA THAT I WANT TO COLLECT (TABULATION OF DATA)
WHAT I CHANGE WHAT I MEASURE
WHAT APPARATUS& MATERIALS ?
1
2 3
4
5
67
8
9
Diagram
40
WHY I DO (AIM)5
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Heat is absorbed or released during a chemical reaction
WHAT I WANT TO CHANGE
MVWHAT IS FIXED
CVWHAT I SHOULD MEASURE
RV
WHEN I CHANGE, WHAT WILL HAPPEN TO WHAT I MEASURE (HYPOTHESIS)
WHY I DO … (AIM) To study ………………..
METHOD I USE ………………
PRO EDURE
DATA THAT I WANT TO COLLECT (TABULATION OF DATA)
WHAT I CHANGE WHAT I MEASURE
WHAT APPARATUS& MATERIALS ?
1
2 3
4
5
67
8
9
Diagram
41
WHY I DO (AIM)5
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Heat is absorbed or released during a chemical reaction
TYPE OF SUBSTANCE
MV WHAT IS FIXED
CVWHAT I SHOULD MEASURE
RV
WHEN I CHANGE, WHAT WILL HAPPEN TO WHAT I MEASURE (HYPOTHESIS)
WHY I DO … (AIM) To study ………………..
METHOD I USE ………………
PRO EDURE
DATA THAT I WANT TO COLLECT (TABULATION OF DATA)
WHAT I CHANGE WHAT I MEASURE
WHAT APPARATUS& MATERIALS ?
1
2 3
4
5
67
8
9
Diagram
42
WHY I DO (AIM)5
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Heat is absorbed or released during a chemical reaction
TYPE OF SUBSTANCE MV
WHAT IS FIXED
CVFinal Temperature
RV
WHEN I CHANGE, WHAT WILL HAPPEN TO WHAT I MEASURE (HYPOTHESIS)
WHY I DO … (AIM) To study ………………..
METHOD I USE ………………
PRO EDURE
DATA THAT I WANT TO COLLECT (TABULATION OF DATA)
WHAT I CHANGE WHAT I MEASURE
WHAT APPARATUS& MATERIALS ?
1
2 3
4
5
67
8
9
Diagram
43
WHY I DO (AIM)5
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Heat is absorbed or released during a chemical reaction
TYPE OF SUBSTANCE
MVWHAT IS FIXED
CVFinal Temperature
RV
Heat is absorbed or released during a chemical reaction.
WHY I DO … (AIM) To study ………………..
METHOD I USE ………………
PRO EDURE
DATA THAT I WANT TO COLLECT (TABULATION OF DATA)
WHAT I CHANGE WHAT I MEASURE
WHAT APPARATUS& MATERIALS
1
2 3
4
5
67
8
9
Diagram
44
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Heat is absorbed or released during a chemical reaction
TYPE OF SUBSTANCEMV
WHAT IS FIXED
CVFinal Temperature
RV
Heat is absorbed or released during a chemical reaction.
To study that heat is absorbed or released during chemical reaction
METHOD I USE ………………
PRO EDURE
DATA THAT I WANT TO COLLECT (TABULATION OF DATA)
WHAT I CHANGE WHAT I MEASURE
WHAT APPARATUS& MATERIALS
1
2 3
4
5
67
8
9
Diagram
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Heat is absorbed or released during a chemical reaction
TYPE OF SUBSTANCE MV
WHAT IS FIXED
CVFinal Temperature
RV
Heat is absorbed or released during a chemical reaction.
To study that heat is absorbed or released during chemical reaction
1. Pour 10 ml of distilled water into each test tube A, B & C
and record the initial temperature.
2. Add a spatula of ammonium chloride into test tube B and stir .
3. Add a spatula of sodium hydroxide into test tube C and stir.
4. Maintain test tube A as a control.
5. Record the final temperature in a table.
DATA THAT I WANT TO COLLECT (TABULATION OF DATA)
WHAT I CHANGE WHAT I MEASURE
WHAT APPARATUS& MATERIALS ?
1
2 3
4
5
6
7
8
9
Diagram
47
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Heat is absorbed or released during a chemical reaction
TYPE OF SUBSTANCEMV
WHAT IS FIXED
CVFinal Temperature
RV
Heat is absorbed or released during a chemical reaction.
To study that heat is absorbed or released during chemical reaction
1. Pour 10 ml of distilled water into each test tube A, B & C
and record the initial temperature.2. Add a spatula of ammonium chloride into test tube B and stir .
3. Add a spatula of sodium hydroxide into test tube C and stir.
4. Maintain test tube A as a control.5. Record the final temperature in a table.
DATA THAT I WANT TO COLLECT (TABULATION OF DATA)
WHAT I CHANGE WHAT I MEASURE
test tube,thermometer, spatula,
Ammonium chloride,Sodium hydroxide &
Distilled water
1
2 3
4
5
67
8
9
Diagram
48
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Heat is absorbed or released during a chemical reaction
TYPE OF SUBSTANCE MV
WHAT IS FIXED
CVFinal Temperature
RV
Heat is absorbed or released during a chemical reaction.
To study that heat is absorbed or released during chemical reaction
.
1. Pour 10 ml of distilled water into each test tube A, B & C
and record the initial temperature.
2. Add a spatula of ammonium chloride into test tube B and stir .
3. Add a spatula of sodium hydroxide into test tube C and stir.
4. Maintain test tube A as a control.
5. Record the final temperature in a table.
DATA THAT I WANT COLLECT (TABULATION OF DATA)
WHAT I CHANGE WHAT I MEASURE
test tube,
thermometer, spatula, Ammonium chloride,
Sodium hydroxide &
distilled water
1
2 3
4
5
6
7
8
9
Diagram
Test tube Initial Temperature (oC) Final temperature (oC) AB
8 49
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Heat is absorbed or released during a chemical reaction
TYPE OF SUBSTANCE
MVVolume of distilled water
CVFinal Temperature
RV
Heat is absorbed or released during a chemical reaction.
To study that heat is absorbed or released during chemical reaction
1. Pour 10 ml of distilled water into each test tube A, B & C
and record the initial temperature.
2. Add a spatula of ammonium chloride into test tube B and stir .
3. Add a spatula of sodium hydroxide into test tube C and stir.
4. Maintain test tube A as a control.
5. Record the final temperature in a table.
DATA THAT I WANT COLLECT (TABULATION OF DATA)
WHAT I CHANGE WHAT I MEASURE
test tube,
thermometer, spatula,
Ammonium chloride,Sodium hydroxide &
distilled water
1
2 3
4
5
6
7
8
9
Diagram
Test tube InitialTemperature (oC) Final temperature (oC)
A
BC
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a. Hypothesis : Heat is absorbed or released during a chemicalreaction depends on type of substances used
b. i. Aim : To study that heat is absorbed or released during a
chemical reaction
ii. Variables :manipulated : type of substances
responding : Final temperature
constant : volume of distilled water//Initial temperature
iii. Apparatus & materials : test tube, spatula, thermometer,ammonium chloride, sodium hydroxide and distilled water.
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iv. Procedure :
1. Pour 10 ml of distilled water into each test tube A, B & C
and record the initial temperature.2. Add a spatula of ammonium chloride into test tube B and stir .
3. Add a spatula of sodium hydroxide into test tube C and stir.
4. Maintain test tube A as a control.
5. Record the final temperature in a table.
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TABULATION OF DATA :
TEST TUBE INITIALTEMPERATURE (oC) FINALTEMPERATURE (oC)
A
B
C
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Learning area:
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Learning area:
5. Energy and chemical changes
Learning Objectives :
5.3 Synthesizing the reactivity series of metal
Learning Outcomes :
A student is able to :
•Describe the reactivity of metals with water, diluteacid and oxygen
•Compare and contrast the reactivity of metals with
water, acid and oxygen
•Arrange metals in order of reactivity with water, acidand water
•Identify the carbon in the reactivity series
•Construct the reactivity series of metals based on
reactivity of metal with oxygen 57
A REACTIVITY OF METALS WITH
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The reaction of metal with water will produce
hydrogen gas and alkali
A.REACTIVITY OF METALS WITH
WATER
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• Sodium and calcium (very active metal )
reacts very fast in cold water.
• Magnesium, aluminium and zinc (less
active metal ) reacts with hot water or
steam.
• Non active metals such as gold and silver
do not react with either water or steam.
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Chemical equations
Sodium + Water Sodium + hydrogen
hydroxide
Magnesium + Water Magnesium + hydrogen
hydroxide
For experiment : Refer to
Appendix 160
B. REACTIVITY OF METALS WITH
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DILUTE ACID Some metals react with dilute acid to produce
salt and hydrogen
General equation:
METAL + ACID SALT + HYDROGEN
Magnesium, aluminium and zinc react with dilute
acid
Copper, silver and gold do not react with dilute
acid
61
2 Type of salt produced
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2.Type of salt produced
depends on the type of acid
used.
Examples:
Zinc + sulphuric acid zinc sulphate + hydrogen
Magnesium + sulphuric acid magnesium sulphate + hydrogen
Aluminium + sulphuric acid Aluminium sulphate + hydrogen
62
C REACTIVITY OF METALS WITH OXYGEN
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C. REACTIVITY OF METALS WITH OXYGEN
When heated in ......................, most metals react with
.......................to form ...........................
General equation
The more reactive the metal, the ...........................
the flame produced.
Metal + Oxygen ...........................
air
o xygen metal oxide
br ighter
metal oxide
For experiment : Refer toAppendix 2 63
Th ti it f t l ith
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The reactivity of metals with oxygen
depends on the reactivity series
Metal + Oxygen Metal oxide
+ o xygen
Zinc
Iron
Zinc oxide+ oxygen
Iron oxide
For experiment :Refer to Appendix 3
64
S b l R ti it M t lReaction with Reaction with Reaction with Reaction with
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Symbol Reactivity MetalReaction with
water
Reaction with
steam
Reaction with
acid
Reaction with
oxygen
Most
Reactive Potassium Hydrogen
gas released
Metal
hydroxidesformed
Explosion Explosion
Violent
reaction
Burn brightly
forming oxidesSodium
Calcium
Magnesium No reaction Hydrogen gas
released
Metal oxides
formed
React fast
Hydrogen gas
released
Metal salts
formed
Aluminium No reaction Burn if strongly
heated
Zinc No reaction
Iron No reaction
Tin (Stanum) No reaction No reaction React slowly
Hydrogen gas
released
Metals do not
burn but oxide
layer formedLead No reaction No reaction
Copper No reaction No reaction No reaction
Silver No reaction No reaction No reaction No reaction
Least
Reactive
Gold No reaction No reaction No reaction No reaction
Platinum No reaction No reaction No reaction No reaction
K
Na
Ca
Mg
A l
Zn
Fe
Sn
Pb
Cu
Ag
Au
Pt
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Carbon and reactivity series
• Metal compounds higher up in thereactivity series are more stable (noteasily decomposed by heat).
• These metal compounds can only bedecomposed by electrolysis.
• Example:
Decomposition of sodium chloride byelectrolysis.
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• Compounds of metals lower down in the
reactivity series are less stable and can be
decompose easily by heating.
• These metal oxides can be reduced by
carbon (reducing agent) into metal and
carbon dioxide.• Example:
Zinc oxide + Carbon Zinc +Carbondioxide
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Symbol Reactivity Reaction of metal oxides with carbon
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y y
Mg No reaction
Al No reaction
C
Zn Less active
Fe Active
Sn More active
Pb Most active
Least active
Most active
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Energy andchemical changes
WaterOxygenAcid
Reactivityof metals
with
Reaction of metaloxides with carbon
Extraction of metal oresby carbon
and electrolysis
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REVISION
• Refer Appendix-4
• My Experiment Sheet
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All the best!!!!!!!
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5.4 Applying the concepts
of the reactivity series
of metal
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Learning Objectives :
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Learning Objectives :
• 5.4 Applying the concepts of the reactivity series
of metal
Learning Outcomes :
A student is able to :
• Relate the position of metals in the reactivity series tothe method of extraction of metals from their ores.
• Explain with examples the process of extraction of a
metal from its ore using carbon.
• State the importance of the reactivity series.
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CONCEPTS OF REACTIVITY
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SERIES• A more reactive metal can take oxygen
from the oxide of other less reactive metal
to form the less reactive metal and the
oxide of the more reactive metal.
• Example: Aluminium + iron oxide iron + aluminium oxide
Morereactivemetal
Oxide of lessreactive metal
Lessreactivemetal
Oxide of moreReactive metal
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• A more reactive non-metal (carbon)
also can take oxygen from the oxide of
other less reactive metal to form theless reactive metal and carbon dioxide.
• Example:
Carbon + iron oxide iron + carbon dioxide
Morereactivenon-metal
Oxide oflessreactivemetal
Lessreactivemetal
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Extraction of metals
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Extraction of metalsMetal Extraction method
Potassium
Electrolysis
Sodium
Calcium
Magnesium
Aluminium
Carbon
Zinc
By heating the ore with carbon
in a furnace
Iron
Tin
LeadCopper Heating the ore alone
Mercury
Silver Exist in metal form
Gold 78
EXTRACTION OF TIN FROM TIN ORE (CASSITERITE)
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1400 o C
1000 o C
400oC
200 o C
Slag is used as
road surfaces
Sulphur + arsenic
Sulphur dioxide + arsenic oxide
Tin ore + carbon
Tin +Carbon dioxide
Blast furnace
Liquid tin is collected
at bottom of furnace
Hot air
limestone
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All the best!!!!!!!
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INSTRUCTION
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1 Teacher introduces the topic with the aid of Diagram 1.
2 Students find the definition of every terminology involved
with the aid of guided worksheet 1.
3 Teacher explains one example of electrolysis of molten
lead(II) bromide. (Refer slide 5)
4 Based on the example above, students try out electrolysis of
molten copper(II)chloride.(Refer slide 6)
5 Students in each group collect and gather information aboutthe uses of electrolysis by using text book or reference book.
(Refer slide 8 – 13)
6 Teacher facilitates students and discusses answers.
7 Students are tested verbally on the learning outcomes.(Refer slide14-19)
8 Students in each group develop a mind map, starts with the
main ideas of electrolysis. (Refer slide 20)
9 At the end of the lesson, students do the self test.
(Refer slide 21 -23)81
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5.5. UNDERSTANDING
ELECTROLYSIS
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1 State what electrolysis is
2 State what anode, cathode, anion, cation and
electrolyte are
3 Describe the electrolysis of an electrolyteusing carbon electrodes
4 Explain the uses of electrolysis in industry
5.5. UNDERSTANDING ELECTROLYSIS
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5.5 ELECTROLYSIS
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A
anion
CathodeAnode
Cation
Electrolyte
Rheostat
Ammeter
Switch
Diagram 1
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Worksheet 1
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•Electrolysis
•Electrolyte
•Electrodes
•Cathode
• Anode
•Cations
• Anions
Process of .................................... of substance using .....................
Substance that ........................... when …………… passes through.
Substance that allow electricity to.................. or ..................
an electrolyte.
The ............................... electrode
The ................................. electrode
.......................... charged ions
........................... charged ions
Meaning of Electrolysis
decomposition electricity
decomposes electricity
enter leave
negative
positive
negatively
positively
Electrical energy ……………… ?
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The Experiment
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The Experiment
Electrolysis of molten lead (II) bromide
Lead
Bromine
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2. Electrolysis of molten lead (II) bromide
Anode Cathode
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Anode Cathode
The .............................. charged
..................... ions move to the anode
The .............................. charged
..................... ions move to thecathode
....................... ions release
.......................... to the anode and form
...............................molecules
................... ions receive
.........................from the cathode and
become ........................ atom.
............. ion + .............
................molecules
................. + electron
…........atom
............. bromine atoms form one
bromine molecule
Lead metal is ............................. on
the ...................
negat ively
bromide
posi t ive ly
lead
Bromide
electrons
bromine
Lead
electrons
lead
Bromide
bromine
electron Lead ion
Lead
Two deposi ted
cathode
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2. Electrolysis of molten copper (II) chloride
Anode Cathode
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Anode Cathode
The .............................. charged
..................... ions move to the anode
The .............................. charged
..................... ions move to thecathode
....................... ions release
.......................... into the anode and
form ...............................molecules
................... ions receive
.........................from the cathode and
turn into ........................ atom.
............. ion + ..............
...............molecules
..................... + electron
…............. atom
............. chlorine atoms form one
chlorine molecule
Copper metal is .............................
on the ...................
negat ively
chlor ide
posi t ive ly
copper
Chlor ide
electrons
chlor ine
Copper
electrons
copper
chlor ide
chlor ide
elect ron copp er ion
copper
Two deposi ted
cathode
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USES OF ELECTROLYSIS IN INDUSTRY
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A. Electroplating
Objects made of iron .................. easily when exposed to air.
To ........................... iron objects from corrosion, they are……………
with a thin layer of non reactive metal such as copper.
The aims of electroplating are to make objects more .......................
and .................. to corrosion.
corrode
prevent coated
attractive
resistant
Click for
experiment
96
• The figure shows an iron spoon being
electroplated with copper .
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A
p pp
i) An iron spoon is used as the ........................
ii) Copper is used as the ..............
iii) The electrolyte is a solution of ......................
compound
• At the anode :
The copper dissolves forming
............................charged copper ions.
• At the cathode:
The .................... ions receive electrons,
forming a coat of ...................... on iron spoon.
• A rheostat is used to control the current flow in
the circuit so that a ..................... and steady
current is used. This is to ensure that the coating
is .......................... and ......................
Copper
as anode
Iron sp oon
Copper s ulphate
so lu t ion
cathode
anode
copper
posi t ive ly
copper
copper
smal l
f i rm even
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NON-REACTIVE METALS SUCH AS
COPPER , SILVER AND GOLD
ARE FOUND AS FREE ELEMENTS.
THESE METALS
CONTAIN IMPURITIES AND CAN BE
PURIFIED BY ELECTROLYSIS
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THE IMPURE METAL IS THE ANODE
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THE PURE METAL OF THE SAME TYPE IS
THE CATHODE
THE ELECTROLYTE IS THE METAL SALT SOLUTION
CONSISTING OF METALLIC IONS WHICH
IS TO BE PURIFIED
IN THE PURIFICATION OF COPPER;
The impure copper is used as anodeThe pure copper is used as cathode
The electrolyte is copper sulphate solution99
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B. Extraction of metals
d b
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Oxygen g ases
Molten
a lumin ium
anode carbon
Cathode
carbon
Baux ite +
cryol i te
115
At th th d
B. Extraction of metals
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Electrolysis is a process to extract metals
such as sodium, ...................... and
aluminium which are more ....................
than carbon.
Aluminium is extracted through
electrolysis from molten
..............................
At the cathode
i) The positively charged .......................
ions are attracted to the cathode.
ii) Aluminium ions receive electrons
and become aluminium ......................
At the anode:
i) The negatively charged
..................... ions are attracted to the
anode.
ii) Oxide ions release electrons to
become ................... atoms
iii) The oxygen atom pairs together to form
… ............ gas
magnes ium
bauxite
reactive
a lumin ium
atoms
oxide
oxygen
oxygen
DIAGRAM
116
A C. Purification of metals
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A
Mass of anode
.................. Mass of
cathode
.................Impuri t ies
decreases
increases
Copper
sulphate
so lu t ion
Anode(impu re cop per)
Cathode
( Pure copper)
117
The diagram shows how electrolysis is used to purify copper
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• The anode is made of ……………………..
• The cathode is made of ……………………..
• The electrolyte used is ………………………..
• When electricity is passed through the electrolyte:
i) The copper anode dissolves to form …………. ions
ii) The positively charged copper ions are attracted to
the ………………………
iii) Copper ions receive electrons from the …………….
and form copper atoms which are deposited on the
…………………
iv) At the same time the …………………… settle to the bottom
impu re copp er
pure copper
copper sulphate solut ion
copper
cathode
cathode
cathode
impur i t ies
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DISCUSSION
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123
**TASK 1
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Label the diagram above. 124
**TASK 2
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Choose the correct answer. 125
**TASK 3
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DRAW YOUR OWN MIND MAP !!!
* MAIN IDEA:
“USES OF ELECTROLYSIS” 126
ELECTROLYSIS is a process of breaking down chemical substances in aqueous
solution or molten state to its constituents by using …………………..
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Electrical energy ……….......... energy
G …………….
EXAMPLE:
Aluminium ion + electrons Aluminium atom
Oxide ion Oxygen atom + electron
(At cathode):
(At anode): 127
(molten aluminium oxide)
ELECTROPLATING IRON NAIL WITH COPPER
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Name of process : ……………………………..
Metal M: ……………………………………...
Electrolyte,N: ………………………………..
ANODE: ………………… CATHODE: …………………….
Metal becomes
……………..
Iron nail is coated
with …………….. layer.
**To obtain a good quality:
1. Dilute ……………… should be used.
2 Use …………….. electric current.
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5.6 Understanding the production
of electrical energy from chemicalreactions
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Learning Objectives
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Learning Objectives
5.6 Understanding the production of
electrical energy from chemical reactions.
Learning Outcomes A student is able to :
i) Describe how a simple cell works
ii) List the various types of cells and theiruses
iii) State the advantages of and
disadvantages of various types of cells
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SIMPLE CELL
• Electrochemical
cell 1
136
THE PRODUCTION OF ELECTRICAL ENERGY BY A
SIMPLE CELL
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Zinc
plate
G
........................................................
................
........................Copper
plate
A simple cell consists of two
....................... and an...........................
Two electrodes made of two different
...............
The electrolyte can be a ..........................,
....................... or ...............................
The diagram shows a simple cell circuit.
In the cell,
i) .................... and copper plates are usedas .....................
ii) ................ is more reactive than copper
iii) The electrolyte used is ..............................
electrodes electrolyte
sal t solut ion
di lu te acid
metals
di lu te alkal i
Z inc
electrodes
Zinc
co pp er (II) su lph ate
so lu t ion
copper (II) sulp hate solut io n
Cont 4
Cont
137
EXERCISE 1• In a simple cell, the more reactive metal acts as the
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In a simple cell, the more reactive metal acts as the......................... terminal which gives out electron and theless reactive metals acts as the ...................... terminal.
• In this process, the zinc plate is the ................... electrodeand the copper plate is the ...................... electrode.
• The .................. from the zinc atoms flow to the copperelectrode through the connecting wire. Thus the ..................electrode dissolves in the electrolyte.
• At the copper electrode , ........................ ion from the
electrolyte receives the electrons.
• The flow of electron from ..................electrode to ...............electrode through the connecting wire deflect thegalvanometer. This proves that the process produces
energy
negat ive
posi t ive
zinc
electrons
hydrogen
posi t ivenegat ive
electr ical
posi t ive
negat ive
138
CELL AND THEIR USAGE Type of cells Uses Advantages Disadvantages
Dry cells
Transistor radio Light Non-rechargeable
N l l i
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Dry cells ..............................
...
..............................
....
..............................
.....
............................
............................
..............................
..............................
............................
............................
..............................
Wet cells ..............................
....
......................................
.....
......................................
......
......................................
......
............................
............................
..............................
..............................
Alkaline
batteries
..............................
....
……………………
….
……………………
......................................
...
......................................
...
......................................
...................................
..
Remote contro l
A larm c lock
Small
Portable
Cheap
Not long last ing
Leakage may happen
Used in vehic les
Rechargeable
High vo l tage
Long- last ing
Heavy
Expensive
Ac id m ight sp i l l
Dist i l led water need to
be addedRadios
Torchl ights
Toys
Large current
Long- last ing
Constant vo l tage
Watches,
Calculators,
Hearing aids
Cameras
Non-rechargeable
Small , long-last ing
Portable
Steady voltage
Constant current
Non-rechargeable
Expensive
ExpensiveRechargeable
Long- last ing
Use in electronic
devices such as
d i i tal camera
ADV 5
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GOOD LUCK
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5.7 LIGHT AND
CHEMICALREACTIONS
CLICK
HERE 146
LE RNING RE
ENERGY AND CHEMICAL CHANGES
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LE RNING OBJECTIVES
1.7 Understanding chemical reactions that
occur in the presence of light
LE RNING OUTCOMES
A student is able to•give examples of chemical reactions which
require light,
•explain the effect of light on photosensitive
chemicals,•explain why certain chemicals are stored in
dark bottles.
147
INSTRUCTIONS:
1.Teacher distributes mahjung paper, marker
d W k h t 1
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pen and Worksheet 1.
2.Teacher groups the students and asksthem to make a Mind Map. Then answer the
questions in Worksheet 1 (Time given : 30
minutes)
3.Teacher facilitates students in their work.4.Teacher will discuss the mind map the
students have done.
5.Teacher will use this power point and the
teaching courseware from PPK duringdiscussion.
148
MIND MAP
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Light and ChemicalReactions
Chemical Changes Caused
by Light EnergyLight Energy and
Photographic Film
Storing Photosensitive
Chemicals
CLICK
HERE 149
Examples of photosensitive chemicals
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• Examples of photosensitive chemicals
Silverbromide
Silverchloride
Hydrogenperoxide
150
Photosensitive Chemicals
Some chemicals are to light
sensi t ive
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Some chemicals are .................. to light .
The chemicals will ................... when ........................ to light.
Examples of photosensitive chemicals are .................................... and
............................................
The chemicals cannot be .................. in a glass bottle.
Hydrogen peroxide .................. + ...........
In the presence of ......................... ,hydrogen peroxide ...................... into
..................... and ..............
Silver chloride ...................... + ...............
Silver chloride decomposes into ........................... and ..........................The chemicals are stored in an ..................... glass bottle.
decompose exposed
hydrogen perox ide
si lver n i t rate
stored
water oxygen
l ight
si lver
decomposes
water oxygen
ch lor ine
si lver ch lor ine
opaque
151
Photosynthesis
Water and
mineral sal ts
are absorb ed
Instructions : Students are asked to answer the questions inWorksheet 2 after discussion.
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................................ + .................................. ............................ + .............................
During photosynthesis, ...................
(green pigment) absorbs ..........................
The energy is used to ............. the .
..................... molecules into
....................... and .......................
.........................is released into the
...............................
The ........................ atoms reacts with
carbon dioxide to form .........................
.................Oxygen is
released into the
air
l ight energy
Carbon dioxide
is abso rbedf rom the air
Glucose
is sent
to the
whole
plant
are absorb ed
from the soi l
by the roots
Water Carbon dioxid e Glucose Oxygen sun l igh t
Chlorophy l l
ch lorophy l l
l ight energy
spl i t
water
hydrogen oxygen
Oxygen
air
hydrogen
glucose
152
PHOTOSYNTHESIS
carbon
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……………
+ ……………. …………….
+ ……………….
chlorophyllcarbon
dioxide oxygen glucose water
…………………
…………………………. Sunlight
153
carbon
dioxide water oxygen glucose
LEARNING OUTCOMES
A student is able to;
explain the effect of light on photosensitive chemicals
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• explain the effect of light on photosensitive chemicals,
• explain why certain chemicals are stored in dark bottles.
Instruction: Teacher directs the students to carry out the group
activity.
Aim : To study the effect of light on chemical reactions
1 Students carry out an activity in groups to study the
effect of light on photographic paper
2 Teacher distributes a piece of photographic paper to
each group.
3. Students place a leaf on the photographic paper and
put it in the sunlight.4. After 10 minutes, students record their observations.
5. Students discuss the effect of light on photographic
paper and present their findings.
154
f O
Observation
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Part of photographic paper Observation
Covered with leaf
Exposed to light
Analysis
1. What inference can be made from your observation?
2. Write a word equation for the reaction of silver bromide with light.
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Photographic paper
Instructions : Students are asked to answer questions in
Worksheet 3 after discussion.
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Silver bromide ...................... + ...............
(Grey)
Photographic paper is coated with ......................... .
When ............... falls on the paper, silver bromide is
.......................... into ........................... and ....................... .
The formation of .................... atoms on the photographic
paper causes....................... black areas on the paper.
Bromine
Photographic paper
s i lver brom ide
decomposed
l ight
si lver
bromine si lver
greyish
Silver
157
Storage of
chemical
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c e ca
substances
The chemicals are stored in
opaque containers or dark
coloured bottles.
CLICK
HERE 158
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5.8 THE BENEFITS OF
CHEMICALREACTIONS
164
LEARNING AREA : ENERGY
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AND CHEMICAL CHANGES
5.8 Appreciating the innovative
efforts in the design of
equipment using chemical
reactions as sources of energy
165
LEARNING OUTCOMES
A student is able to :
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A student is able to :
- describe how energy obtained from chemical
reactions should be used efficiently to prevent
wastage
- describe how equipment utilising chemical reactions
as sources of energy should be disposed to reduceenvironmental pollution
- give suggestions on new ways of using chemical
reactions as sources of energy for equipment
- put into practice good habits when using anddisposing equipment that uses chemical reaction as
a source of energy166
CONTENT OF THESE LEARNING OUTCOMES
- equipments using chemical reactions
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- efficient use to prevent wastage
- proper disposal- alternative sources of energy
- use energy saving electrical appliances
- iron all the clothes at one time- turn off all electrical appliances when not in
use
- use fluorescent lamps instead of bulbs- close refrigerator door as soon as possible
- (other possible answers)167
Group Work : Students do a
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mind map on the innovativeefforts in the design of
equipment using chemicalreactions as sources of energy
linking all the learning
outcomes.
168
Students can obtain theinformation from websites,
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,
books, magazines, journals ornewspapers.
(Note : An example is shownbelow)
#Slides 13,14,15 are motivational slides, to be
used when needed.169
Mind map Equipments
using
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Efficient useto prevent
wastage
ProperDisposal
Alternative
sources of
energy
us g
chemical
reactions
# continue next
slide
170
Efficient use to
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Use energy
saving
electrical
appliances
Iron all theclothes at
one time
Turn offelectrical
appliances
when not in use
prevent
wastage
171
Proper
Used
batteries
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Disposal
172
Alternative
sources of
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sources of
energy
173
SELF TEST1. Cellular phones use …………….
batteries.
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batteries.
2. Name two appliances that useelectrical energy.
3. Name the gas produced from the
burning of fossil fuels that can cause acidrain.
4. Name a way you can help to conserve
electricity in your home.
5. What happens when toxic substancesare not disposed off properly?
174
Answers to Self Test
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Answers to Self Test1. rechargeable2. toaster, computer, television
3. sulphur dioxide
4. Turn off the lights when not in use.5. Toxic substances if not disposed off
properly will cause environmental
pollution.
175
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Education isnot preparation
for life;education is lifeitself.
176
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MARIA MITCHELL: Study as if you
were going to live
forever; live as if
you were going to
die tomorrow..
177
• FRANCIS BACON:
• We cannot command nature
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except by obeying her.
• LINDA HOGAN: • There is a way that nature
speaks, that land speaks. Most of
the time we are simply not patientenough, quiet enough, to pay
tt ti t th t
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