Summary organic chemistry, rate of reaction

Chemical kinetics = how fast reaction takes place

thermodynamics -_
whether or not reactions take place


COLLISION THEORY OF CHEMICAL REACTION
rate of reaction =
largely affected by the concentration of reactant and temperature
→ rate ↑ when number of collisions ↑ Is
potential energy =
energy stored in the bonds within and among the particles of the
reactants
kinetic energy __
movement of the particle
activation energy =
minimum amount of energy required to initiate a chemical reaction
potential energy
☐

a-
- . . . . . . . . .
* EXOTHERMIC reaction

/Ea
/ www.mtnanreao-ant
-
_ activation potential energy of the product is lower
- - ⇒ _
ever ☐
Ea for backward



☐ reaction pathway

REACTION RATE
change in the concentration ofareactan-oraprodnc-wi-hti.me
=



rate ☐ [ A]= * change in concentration OFA overtime
-




of

=
☐ [B) * change in concentration OFB overtime
of

negative rate __ concentration of substance decrease overtime
↳
rate law =K[ A) WEB ] 's
neactionqgp~itdlfimshowmuchttera-e.is
affected
↳ N + D= overall by changes in the concentration Ofa reactant
↳ K =
rate constant


EXPERIMENTAL DETERMINATION OF THE RATE LAW
1=2191+26102 (g) 021=610219 )
experiment F2 1MI Close 1Mt initial rate IMIS )
I 0.1 0.010 I -2×10-3
2 0.1 0.040 4.8×10-3
3 0.2 0.010 2.4×10-3
"
experiment } =
k[ Fz ] [ CIOZIY experiment 2 =
K [ Fz ]k[ C10 ≥ ] "

experiment I K1T-2IR [ CE02 ] 's experiment / KE1-2IU [ C10 2IY
2. 4×10-3 =
K10 2) 110.1019
- 4.8×10-3 =
K10-0IO )k 10.040 )
"


I. 2×10-3 K10 / IN 10.1019. I -2×10-3 K10 -0101mL 0.01019

2=2
"
4 = 49

k=I ,
with respect -101=2 D= I
,
with respect -10402

÷ rate of law = I + I
=
2