IB Chemistry Topic 6 Kinetics 16.1 Rate expression and reaction mechanism
Exploration of chemical kinetics using experimental data to determine reaction orders and mechanisms
Full resources for topic 6: www.mrwengibche...
0:23 The rate equation
0:32 Order of reaction
1:13 Units for the rate constant k
2:26 Graphical determination of rate
2:46 Determining order with concentration vs time graph
3:45 Determining order with rate vs concentration graph
5:04 Rate of reaction calculations
6:12 Reaction mechanisms
8:17 Unimolecular vs bimolecular steps
8:59 Intermediate vs transition states
9:29 Enthalpy diagram: Intermediate vs transition states
10:05 Determining order of reaction from reaction mechanisms
11:26 Practice problems
16.1 Rate expression and reaction mechanism HL
• Reactions may occur by more than one step and the slowest step determines the rate of reaction (rate determining step/RDS).
• The molecularity of an elementary step is the number of reactant particles taking part in that step.
• The order of a reaction can be either integer or fractional in nature. The order of a reaction can describe, with respect to a reactant, the number of particles taking part in the rate-determining step.
• Rate equations can only be determined experimentally.
• The value of the rate constant (k) is affected by temperature and its units are determined from the overall order of the reaction.
• Catalysts alter a reaction mechanism, introducing a step with lower activation energy.
• Deduction of the rate expression for an equation from experimental data and solving problems involving the rate expression.
• Sketching, identifying, and analysing graphical representations for zero, first and second order reactions.
• Evaluation of proposed reaction mechanisms to be consistent with kinetic and stoichiometric data.
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