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IB Chemistry Kinetics Topic 6.1 Collision theory and rates of reaction
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IB Chemistry Kinetics Topic 6.1 Collision theory and rates of reaction
Using the collision theory to understanding the kinetics of reaction rates
0:00 Collision theory Spartan version
1:01 Collision theory IB version
1:50 Enthalpy diagram activation energy
2:33 Reaction rates: Collision rate vs activation energy
2:55 Reaction rates: Concentration
3:37 Reaction rates: Surface area
4:25 Reaction rates: Temperature
5:05 Maxwell-Boltzmann curve with temperature
6:10 Reaction rates: Catalysts
6:36 Maxwell-Boltzmann curve with catalysts
7:04 Enthalpy diagram with catalysts
7:17 Rate of reaction formula
7:34 Preparing for rates of reaction experiments
8:19 Rate of reaction experiments: Gas collection
9:08 Rate of reaction experiments: Change in mass
9:32 Rate of reaction experiments: Spectrophotometry
9:54 Rate of reaction experiments: pH or conductivity
10:41 Rate of reaction experiments: Clock reactions
10:52 Rate of reaction graph and calculations
6.1 Collision theory and rates of reaction SL
• Species react as a result of collisions of sufficient energy and proper orientation.
• The rate of reaction is expressed as the change in concentration of a particular reactant/product per unit time.
• Concentration changes in a reaction can be followed indirectly by monitoring changes in mass, volume and colour.
• Activation energy (Ea) is the minimum energy that colliding molecules need in order to have successful collisions leading to a reaction.
• By decreasing Ea, a catalyst increases the rate of a chemical reaction, without itself being permanently chemically changed.
• Description of the kinetic theory in terms of the movement of particles whose average kinetic energy is proportional to temperature in Kelvin.
• Analysis of graphical and numerical data from rate experiments.
• Explanation of the effects of temperature, pressure/concentration and particle size on rate of reaction.
• Construction of Maxwell–Boltzmann energy distribution curves to account for the probability of successful collisions and factors affecting these, including the effect of a catalyst.
• Investigation of rates of reaction experimentally and evaluation of the results.
• Sketching and explanation of energy profiles with and without catalysts.
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Using the collision theory to understanding the kinetics of reaction rates
0:00 Collision theory Spartan version
1:01 Collision theory IB version
1:50 Enthalpy diagram activation energy
2:33 Reaction rates: Collision rate vs activation energy
2:55 Reaction rates: Concentration
3:37 Reaction rates: Surface area
4:25 Reaction rates: Temperature
5:05 Maxwell-Boltzmann curve with temperature
6:10 Reaction rates: Catalysts
6:36 Maxwell-Boltzmann curve with catalysts
7:04 Enthalpy diagram with catalysts
7:17 Rate of reaction formula
7:34 Preparing for rates of reaction experiments
8:19 Rate of reaction experiments: Gas collection
9:08 Rate of reaction experiments: Change in mass
9:32 Rate of reaction experiments: Spectrophotometry
9:54 Rate of reaction experiments: pH or conductivity
10:41 Rate of reaction experiments: Clock reactions
10:52 Rate of reaction graph and calculations
6.1 Collision theory and rates of reaction SL
• Species react as a result of collisions of sufficient energy and proper orientation.
• The rate of reaction is expressed as the change in concentration of a particular reactant/product per unit time.
• Concentration changes in a reaction can be followed indirectly by monitoring changes in mass, volume and colour.
• Activation energy (Ea) is the minimum energy that colliding molecules need in order to have successful collisions leading to a reaction.
• By decreasing Ea, a catalyst increases the rate of a chemical reaction, without itself being permanently chemically changed.
• Description of the kinetic theory in terms of the movement of particles whose average kinetic energy is proportional to temperature in Kelvin.
• Analysis of graphical and numerical data from rate experiments.
• Explanation of the effects of temperature, pressure/concentration and particle size on rate of reaction.
• Construction of Maxwell–Boltzmann energy distribution curves to account for the probability of successful collisions and factors affecting these, including the effect of a catalyst.
• Investigation of rates of reaction experimentally and evaluation of the results.
• Sketching and explanation of energy profiles with and without catalysts.
Connect with me:
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