Chemical Kinetics Flashcards
Gibb’s free energy
Determines spontaneity
Mechanism
Steps of the reaction
Rate of the whole reaction is only as fast as
The rate-determining step
Collision theory of chemical kinetics
The rate of reaction is proportional to the number of collisions per second between reacting molecules with correct orientation and with enough energy to break existing bonds and form new ones
Activation energy/Ea
minimum energy of collision necessary for a reaction to take place
Rate=
Z x f
Z=collisions/sec
f=fraction of collisions that are effective
Arrhenius equation
k=Ae^-E/RT
k=rate constant
A=frequency factor
R=ideal gas constant
Frequency factor (A)
Measure of how often molecules in a certain reaction collide in s^-1
As temperature increases, what happens to rate constant
Increases, less negative exponent means more positive and larger
Transition state/Activated complex
Has greater energy than reactants or porducts
Transition state v. Reaction intermediate
Transition state is only theoretical
free energy change of the reaction
Difference between the free energy of products and reactants
Transition state between to products and to reactants
On either side of the transition peaks
What measures the concentration of gases of gas reactants
Partial pressures
Effect of temp on reaction rate
Almost always increases
Raising a reaction 10 C usually does what?
Double the rate of the reaction
Why would a polar solvent be preferred
Molecular dipole polarizes bonds of reactants
