Powerpoints: 0_significant_digits.pdf , 1.monitoringrates.ppt , 2.factorsthatincreaserate.ppt , 3.collisiontheory.ppt , 4_energy_change.ppt , 5.potentialenergydiagrams.ppt , 6.mechanisms.ppt , 7.catalysts.ppt , 8.Review.ppt ,
Worksheets: 1-0.pdf , 1-0key.pdf , 1-2.pdf , 1-2key.pdf , 1-3.pdf , 1-3key.pdf , 1-4.docx , 1-4key.docx , 1-5.pdf , 1-5key.pdf , 1-6.pdf , 1-7ReviewQuiz.pdf , 1-7ReviewQuiz2.pdf , KEDistrubutin class Questions.docx , checklist.pdf , collision theory.docx , designlab.docx , factors affecting reaction rates.doc , rate of reaction.doc , unity is strength.docx , worksheets.htm ,
1 .2 Methods Of Measuring Reaction Rates
1. Rate = △Colour intensity/△time
2. Rate = △temperature/△time
3. Rate = △pressure/△time
4. Rate = △mass/△time
5. Learned the diagram of a simple spectrophotometer (use to measured colour)
1 .3 Factors Affecting Reaction Rates
1. When temperature increases, the time required for the reaction decreases. But, a decrease in the time for the reation is caused by an increase in the rate, so that when the temperature increase, the rate increases.
2. As reactant concentration increases, the time required for the reaction decreases. Hence, when reactant concentration increases the reate increasers.
3. When the pressure of a gaseous reactant increases, more of the reactant is compressed into a given volume (that is ,the reactant concentration increases). Hence, when the reeactant pressure increases, the rate increases.
4. Some reactions are naturally slow because the bonds involved are very strong and unreactive, or the electrons involved are tightly held. Other reactions are naturaally fast because the reaction involves breaking weak bonds or removing loosely-held electrons. Chemist have no control over these fundamental differences in the rates of reactions.
5. The NATURE OF THE REACTANT is the term used to describe the chemical properties of a substance.
Labs: rate change analysis.doc ,
1 .4 I.4 Experimental Measurement Of Reaction Rates & I.5 Reaction Rates And Collision Theory
1. We learn that the calculation of reaction rate is using : Rate=slope= rise/run.
2. The amount of reactants will influence the average reaction rate. For example: less reactants will have less average rate.
3. We learn that the collision theory is also called Kinetic Molecular Theory.
4. The collision theory states that molecules act as small, hard spheres which bounce off each other and transfer energy among themselves during their collisions.
5. The effect of concentration and the effect of temperature are the conditions of the reaction.
Tutorial Videos: 1-4reaction rates.mp4 ,
1 .6 Enthalpy Changes In Chemical Reaction
1. We learn that what is potential energy and how can they show it in the graph. In the potional energy diagram the x-value is reaciton proceeds and y-vaule is potential energy.
2. In the reaction when the chemical is breaking bonds we must add energy, otherwise, forming bonds release energy.
3. Entalpy is the total energy (kinetic and potential)which exists in a system when at constant pressure.
4. Exothermic reaction loss energy to the surroundings.
5. Endothermic reaction take energy from the surroundings.
1 .7 Kinetic Energy Distributions
1. For slow reaction, a 10℃ temperature increased doubles the rate.
2. For a slow reaction there must be an intermidiate energy
3.As the temperature of the system ia increased, the average energy of the system is increased.
4. The reaction rate is slow in room temperature because only few molwcules have sufficient energy to react.
5. Temperature changing kinetic energy distribution graph
Tutorial Videos: 1-7ADistribution of Kinetic Energy - YouTube_标清.flv , 1-7B 6.2.5 Explain Qualitatively the M-B Energy Distribution Curve IB Chemistry SL.flv , 1-7cChemFlick 1-12 Kinetic Energy Distributions._标清.flv ,