1. 6. Graphs and Data Interpretation
1.1. 6.1 Rate Graphs
1.1.1. Steeper slope = faster reaction
1.1.2. Slope represents rate
1.2. 6.2 Analyzing Graphs
1.2.1. Comparing rates from different conditions
1.2.2. Calculating the mean rate of reaction
2. 3. Collision Theory
2.1. 3.1 Key Concept
2.1.1. Collisions must have sufficient energy (activation energy)
2.1.2. Particles must collide to react
2.2. 3.2 Activation Energy
2.2.1. Minimum energy needed for a reaction to occur
3. 1. Factors Affecting Rate of Reaction
3.1. 1.1 Temperature
3.1.1. Particles collide more frequently
3.1.2. Increases kinetic energy
3.1.3. More successful collisions
3.2. 1.2 Concentration
3.2.1. Higher concentration increases collision frequency
3.2.2. More reactant particles in the same volume
3.3. 1.3 Surface Area
3.3.1. Smaller particles have a larger surface area
3.3.2. More area for collisions
3.3.3. More collisions per second
3.4. 1.4 Catalysts
3.4.1. Lowers activation energy
3.4.2. Provides alternative reaction pathway
3.4.3. Not used up in the reaction
3.5. 1.5 Pressure (for gases)
3.5.1. Higher pressure increases collision frequency
3.5.2. Particles are closer together
4. 2. Measuring Rate of Reaction
4.1. 2.1 Methods
4.1.1. Change in mass
4.1.2. Volume of gas produced
4.1.3. Disappearing cross method (precipitation)
4.2. 2.2 Units
4.2.1. cm³/s, g/s, mol/s
5. 4. Reaction Profiles
5.1. 4.1 Energy Diagrams
5.1.1. Activation energy peak
5.1.2. Exothermic vs. Endothermic reactions
5.2. 4.2 Catalysts in Energy Diagrams
5.2.1. Lower peak for activation energy with catalyst
6. 5. Practical Investigations
6.1. 5.1 Core Required Practicals
6.1.1. Measuring how concentration affects reaction rate
6.1.2. Measuring how surface area affects reaction rate
6.1.3. Investigating the effect of temperature on reaction rate
6.1.4. Investigating the effect of a catalyst on reaction rate
6.2. 5.2 Key Observations
6.2.1. Rate changes over time
6.2.2. Different methods of data collection