Chapter 5 - Chemical Kinetics Flashcards
Gibbs free energy (delta G)
Determines if her reaction will occur, negative the reaction will spontaneously occur, and positive reaction will not spontaneously occur
Rate determining step
The slow step. This is used to create the reaction equation
Collision theory of chemical kinetics
The rate of reaction is proportional to the number of collisions per second
Activation energy
The minimum energy occlusion needed for a reaction to occur
Frequency factor
How often molecules in a certain reaction collide
Transitions state
The molecule and reaction that has greater energy than both reactants, the top of the curve. Transition states are not stable molecules.
Free energy change of a reaction
The difference between D initial and final energy state determining if the reaction is Exergonic or endergonic
Exergonic
Negative free energy change, energy is released from the reaction
Endergonic
Positive free energy change in a reaction, energy is absorbed by the reaction
Factors that increase a reaction rate
Higher concentrations of reactants, in reactions above zero order.
Increasing temperature, but not to the point that it denatures proteins that help the reaction along.
Reaction medium, polar solvents tend to polarized the bonds of the reactants, lengthening and weakening the bonds for easier breaking.
Catalysts, not consumed in the reaction, but stabilize intermediates to reduce the activation energy.
Homogenous catalyst
A catalyst in the same phase as the reactants
Heterogeneous catalyst
Catalyst in a different phase from the reactants
Rate law
Rate= k[A]^x[B]^y
Keq
Rate of forward reaction/rate of the reverse reaction.
Zero order reaction
K[A]^0[B]^0
Independent of the concentration of reactants
