6.2 factors affecting rates of reaction
TRANSCRIPT
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Collision Theory
Factors affecting rate
Investigate how concentration affects rate
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Collision Theory
1. For a reaction to occur the particles must collide
2. The colliding particles must have a minimum energy called the
Activation Energy
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Collisions & Activation Energy
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Factors affecting Rate of reaction
1. Concentration
2. Temperature
3. Particle size
4. Nature of reactants
5. Presence of a catalyst
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Effect of concentration on rate
Increasing concentration increases the rate
By increasing the number of collisions
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The formation of a pale yellow precipitate of sulphur can be used to monitor the progress of
the reaction
HCl Na2S2O3 H2O+NaCl
Investigate the effect of concentration on reaction rate
+ + S+ SO2
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To investigate the effect of concentration on reaction rate
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Add the HCl to the Na2S2O3 in the flask
Record the time taken for the X to disappear
Repeat with different concentrations of Na2S2O3 Inverse the time to get the rate
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Effect of concentration on rate
RATE
CONCENTRATION
Conclusion ?
Rate is directly proportional to concentration
1
Time
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Collision Theory
Factors affecting rate
Particle size affects rate
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Collision Theory
1. For a reaction to occur the particles must collide
2. The colliding particles must have a minimum energy called the
Activation Energy
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Factors affecting Rate of reaction
1. Concentration
2. Temperature
3. Particle size
4. Nature of reactants
5. Presence of a catalyst
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Effect of Particle size on rate
Smaller particles have a greater surface area
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Surface area, collisions & rate
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The rate of release of CO2 gas can be used to monitor the progress of the reaction
HCl CaCO3 H2O +
Investigate the effect of particle size on reaction rate
+ + CO2CaCl2
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Add the HCl to a large chips of CaCO3 in the flask
As CO2 is released the mass of the flask drops
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Record the time taken for the release of CO2 to end ( No further mass loss)
Repeat using the same mass of powdered CaCO3
and the same volume of HCl
And the same concentration of HCL
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Result
Finely divided particles react faster than large particles
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Collision Theory
Factors affecting rate
Investigate how temperature affects rate
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Collision Theory
1. For a reaction to occur the particles must collide
2. The colliding particles must have a minimum energy called the
Activation Energy
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Factors affecting Rate of reaction
1. Concentration
2. Temperature
3. Particle size
4. Nature of reactants
5. Presence of a catalyst
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Temperature, Collisions & Activation Energy
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Effect of temperature on rate
Increasing temperature increases the rate
By increasing the number of collisions / sec
More of the colliding particles have E Act
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The formation of a pale yellow precipitate of sulphur can be used to monitor the progress of
the reaction
HCl Na2S2O3 H2O+NaCl
Investigate the effect of temperature on reaction rate
+ + S+ SO2
![Page 24: 6.2 factors affecting rates of reaction](https://reader033.vdocuments.us/reader033/viewer/2022061521/555040a2b4c905b2788b4928/html5/thumbnails/24.jpg)
To investigate the effect of temperature on reaction rate
Next slide
Add the HCl to the Na2S2O3 in the flask
Record the time taken for the X to disappear
Record the temperature after mixing
Inverse the time to get the rate
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Next slide
Repeat at different temperatures
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Effect of temperature on rate
RATE
TEMPERATURE
Conclusion ?
Rate increases with increasing temperature
1
Time
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Effect of temperature on rate
RATE
TEMPERATURE
What is the main factor
increasing rate between A and B
Rate increases due to increased collisions /sec
1
Time
A
B
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Effect of temperature on rate
RATE
TEMPERATURE
What other factor caused the large rate
increase between B and C
More colliding particles have E Act
1
Time
C
B
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Nature of reactants affect the rate
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Collision Theory
1. For a reaction to occur the particles must collide
2. The colliding particles must have a minimum energy called the
Activation Energy
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Factors affecting Rate of reaction
1. Concentration
2. Temperature
3. Particle size
4. Nature of reactants
5. Presence of a catalyst
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Nature of reactants affects rate
Ionic reactions are fast
Na+Cl- Ag+NO3-+ =
Ag+Cl-+
Na+NO3-
Mix solutions of sodium chloride and silver nitrate
A precipitate of silver chloride forms instantly
Ions are free to move in solution....no bonds to break
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Sodium chloride + Silver Nitrate
next
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The pale yellow precipitate of sulphur forms slowly as covalent bonds in the sodium thiosulfate must first
be broken before the reaction can occur
HCl Na2S2O3 H2O+NaCl+ + S+ SO2
Covalent reactions are slower than ionic
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End