2513737
chemical kinetics
- expression of average rate of rxn
- rate law
- rate=k[A][B] or -d[R]/dt=k[A]^x[B]^y
- for eg 2NO +O2----->2NO then
,rate=k[NO]^2[O2]
- for eg 2NO +O2----->2NO then
,rate=k[NO]^2[O2]
- rate=k[A][B] or -d[R]/dt=k[A]^x[B]^y
- order of the rxn
- the sum of powers of concetration of the
reactants in the rate law expression is
called order of the rxn
- units of rate of the rxn
- 1st order rxn=s
- graph of 1nd order rxn
- graph of 1nd order rxn
- zero order rxn =mol L s
- graph of zero order rxn
- graph of zero order rxn
- second order rxn=mol L s
- graph of 2nd order rxn
- graph of 2nd order rxn
- 1st order rxn=s
- the sum of powers of concetration of the
reactants in the rate law expression is
called order of the rxn
- molecularity of a rxn
- the number of reacting species
taking part in an elimentary rxn
which must collide in order to
bring abot a chemical rxn
- the number of reacting species
taking part in an elimentary rxn
which must collide in order to
bring abot a chemical rxn
- integratedrate of equation
- zero order rxn
- k=[Ro]-[R]/t
- Graph
- Graph
- k=[Ro]-[R]/t
- 1ST ORDER RXN
- K= (2.303\T)Log[Ro]\[R]
- graph
- half life =0.0693/k
- graph
- pseudo 1et order rxn
- k'=[HO]K
- k'=[HO]K
- IF All recatant and
produt are gaseous
- k=(2.303/t)log (P i/P a)
then
k=(2.303/t)log(Pi/(2Pi-Pt))
- k=(2.303/t)log (P i/P a)
then
k=(2.303/t)log(Pi/(2Pi-Pt))
- K= (2.303\T)Log[Ro]\[R]
- zero order rxn
- TEMP DEPENDENCE OF
RATE OF RXN
- -Ea/RT
K=Ae ...
- lnk=-(Ea/RT)+Ln(K)
- Ln(K2/k1) = Ea [ T2-T1]
2.303[T1.T2]...
- lnk=-(Ea/RT)+Ln(K)
- -Ea/RT
K=Ae ...
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