Chapter 5 Flashcards
Gibbs free energy
delta G
can it occur without assistance
collision theory
rate of reaction to proportional to the number of collisions per second
must be an effective collision (right orientation, enough energy)
activation energy
Ea, minimum collision energy needed for reaction
KE over Ea= reaction
Reaction rate
= Z x F
z= total collisions per s
F= fraction of effective collisions
Rate constant equation
K= Ae (^-Ea/Rt)
k= rate constant
A= freq. factor
R= ideal gas
t- temp in K
as exponent decreases, it moves towards zero and rate will increase
rate increases with temp and Ea
frequency factor
how often molecules in a reaction collide
transition state
greater energy than reactants and products
to reach TS equals activation energy
what affects reaction rate
increase in conc. of reactants will increase collisions and rate
increase temp will increase KE and increase rate
solution (polar is favored, as dipoles weaken bonds)
Rate formula
-A/ at= -B/bt = C/ct= D/dt
reactants are negative and products are positive
rate law formula
rate= k [A]^x [B]^y
overall order= X + Y…
how to determine rate law
experimentally, when conc of one reactant is unchanged, by what factor is the other changed
zero order
rate of product formation is independent of change in concentrations of reactions
in m/s
change rate using temp or catalyst
k= -slope
first order
rate directly proportional to only one reactant
in 1/s
ln A, k=-slope
radioactive decay
first order
[A]t= [A]0 e^-kt
second order
rate is proportional to concentration of two reactants or square of single reactant
in 1/ms
1/[A]. k= slope
