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Reaction Rates
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Classify the following reactions:
1. Mg + Fe2O3  Fe + MgO
2. NH3 + I2  N2I6 + H2
3. H2O + SO3  H2SO4
4. O2 + C3H8  H2O + CO2
5. CaSO4 + Mg(OH)2  Ca(OH)2 + MgSO4
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Find your seat & Do Now
Classify the following reactions:
1. Mg + Fe2O3  Fe + MgO
2. NH3 + I2  N2I6 + H2
3. H2O + SO3  H2SO4
4. O2 + C3H8  H2O + CO2
5. CaSO4 + Mg(OH)2  Ca(OH)2 + MgSO4
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Find your seat & Do Now
Classify the following reactions:
1. Mg + Fe2O3  Fe + MgO
2. NH3 + I2  N2I6 + H2
3. H2O + SO3  H2SO4
4. O2 + C3H8  H2O + CO2
5. CaSO4 + Mg(OH)2  Ca(OH)2 + MgSO4
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Find your seat & Do Now pg.14
Classify the following reactions:
1. Mg + Fe2O3  Fe + MgO
2. NH3 + I2  N2I6 + H2
3. H2O + SO3  H2SO4
4. O2 + C3H8  H2O + CO2
5. CaSO4 + Mg(OH)2  Ca(OH)2 + MgSO4
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Find your seat & Do Now pg.14
Classify the following reactions:
1. Mg + Fe2O3  Fe + MgO
2. NH3 + I2  N2I6 + H2
3. H2O + SO3  H2SO4
4. O2 + C3H8  H2O + CO2
5. CaSO4 + Mg(OH)2  Ca(OH)2 + MgSO4
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Find your seat & Do Now pg.14
Classify the following reactions:
1. Mg + Fe2O3  Fe + MgO
2. NH3 + I2  N2I6 + H2
3. H2O + SO3  H2SO4
4. O2 + C3H8  H2O + CO2
5. CaSO4 + Mg(OH)2  Ca(OH)2 + MgSO4
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announcements
 JOURNAL CHECK/EXAM 3!!!!
 A-DAY Nov 24
 B-DAY Nov 25
Journal check expectations:
vocabulary flip-chart complete (definitions &
pictures)
Practice/skill assignments complete &
directions have been followed.
Do Now’s are complete
Objective:
 Explain how various factors affect the rate of a chemical
reaction.
What is a chemical change? (2 tix)
CONCEPT MAP (copy this)
 Chemical reaction:
 Rate of reaction:
 Kinetic molecular Theory:
FACTORS THAT AFFECT RATE
Temperature
Surface Area
Concentration
Catalysis
Pressure
CHEMICAL FORMULAS
H2O + SO3  H2SO4
Reactants
The “starting stuff ”
Yeild
Products
The “end result”
CHEMICAL FORMULAS
Mg + Fe2O3  Fe + MgO
Equilibrium:
The reactants are being turned into products at the same rate
as products are being turned into reactants.
Chemical Reaction
 Transformation of one set of chemical substances to
another.
Rate of Reaction
 How fast or slow a reaction takes place.
 It is the decrease in the concentration of the reactants over
time.
Reactants
 Products
Temperature
 ↑ the temperature = Faster motion of particles = more collisions =
faster reaction.
 Example: It’s easier to make sweet tea in
hot water than cold water.
Surface Area
 When you increase surface area, the reaction rate
increases
 Allows particles to come into contact faster, less to
break down
Concentration
 ↑ concentration = increasing # of particles in the
reaction=faster reaction
 Example:
1 person pushing at a car vs. 3 people
PRESSURE
 Increase pressure , increase reaction rate
Catalyst
 Is a substance that speeds up a reaction without
being permanently changed.
 Lowers the activation energy of the reaction so you
have a faster reaction.
 Example:Your saliva
ARE YOU AWAKE?
 Which of the following factors should not have any effect on
the rate of the reaction?
 Temperature
 Density
 Concentration
 Catalyst
ARE YOU AWAKE?
 The rate of reaction refers to
 the amount of reactant present at the start of the
reaction
 the speed of the reaction
 the amount of product produced from the reaction
 How concentrated the reactants are
ARE YOU AWAKE?
 For a given reaction, increasing the temperature would do
what?
 Increase the reaction rate because particles are moving faster
 Decrease the reaction rate because particles are moving faster
 Increase the reaction rate because particle are moving slower
 Decrease the reaction rate because particles are moving faster
KINETIC MOLECULAR THEORY
 Molecules are in constant motion. This motion is
different for each of the three states of matter.
 They are colliding with each other and the walls of their
container.
JOURNAL PAGE ___
C – minimum; you have 5 minutes
H – none
A – Copy Table 18.1: Review of Rate Affecting Factors
M – RAISE YOUR HAND TO GET UP
P – everyone!
SUCCESS!
BRAIN BREAK! (4 tix)
Using only 6 lines, connect all 16 dots.
VIDEO (2:00)
On journal page 18, write…
List the 5 ways to increase “chemical reactions in
schools” :
1. ___________________
2. ___________________
3. ___________________
4. ___________________
5. ___________________
Partner
Practice
*Directions: Write the answers out and 1 sentence
WHY the answer is correct for FULL credit.
C – minimum; on topic only
H – use your notes!
A – Reaction Rates Partner Practice
M – Remain in seat. Raise your hand to get up!
P – everyone!
SUCCESS!
• WHEN YOUR DONE, work on the
measurement/scientific method worksheet
• I will come around and check for Vocab Flip Chart
Exit Slip
 Explain why it takes longer for food to go “bad” in a
refrigerator rather than on the counter.
 3 sentences minimum
Lab Activity
 Bring only your lab papers outside.
 Decide who is going to be the recorder, the timer, and the
engineer in each group.
 Recorder- writes down the data
 Timer- responsible for keeping track of the time for each trial
 Engineer (2)- handles the materials
 Everyone- cleanup
Directions
 Temperature (1 and 2)
 Concentration
 Hot Water (get last)
 Normal Water
 A film canister
 A film canister
 1 alkaseltzer tablet
 2 alkaseltzer tablets
 Surface Area
 Normal Water
 A film canister
 1 alkaseltzer (crushed)
 Control Group
 Normal Water
 Film Canister
 1 alkaseltzer tablet