Chemical Reaction Rates Flashcards
kinetics
how a reaction proceeds and how fast
reaction rate
the change in the concentration of a reactant/product over time (mol/Lxs)
rate of consumption
change in reactants [R] over a period of time (t)
rate of production
change in products over a time period
average rate of reaction
the change in the concentration of a reactant or product per unit over a given time interval
instantaneous rate of reaction
the rate of a chemical reaction at a particular point in time
kinetic molecular theory (KMT)
an increase in temperature
- increases the speed of particles
- reduces the forces of attraction
between particles
collision theory
reactants must collide with one another for a chemical reaction to occur
- collide
- collide with enough of energy
- collide with the right geometry
factors that affect reaction rates are…
concentration, temperature, the nature of reactants, surface area and catalysts
catalyst
increases the reaction rate by producing a different reaction with a lower activation energy. it is not consumed by the reaction
activation energy of forward (Eaf)
difference in energy between reactants and transition state/activation complex
activated complex
the energy required to START the reaction (where the energy is most stable)
activation energy of reverse of RxN (Ear)
difference in energy between products and transition state/activation complex
Heat of RxN (Enthalpy)
difference between reactants and products
reactants < products
endothermic
