Chapter VIII Phenomenological chemical kinetics (empirical/classical) -- experimental aspects 3 The rate equation of reaction with simple order The purposes of the rate law: 1) Given the composition of the reaction mixture, the rate law can predict the reaction rate. 2) Gives clues to the mechanism and testify the proposed mechanism. 3) To classify reactions on the reaction order. It was found that reactions with same reaction order are usually of same kinetic characteristics, therefore, reactions are usually classified on the basis of reaction order. 1 1 r k [H ] [I ] H2 + I2 = 2 HI 2 2 1 0.5 r k [H ] [Cl ] H2 + Cl2 = 2 HCl 2 2 H2 + Br2 = 2 HBr Overall reactions [H 2 ][Br2 ]0.5 rk [HBr] 1 k ' [Br2 ] Reaction with definite order Reaction without definite order Reaction with simple order Reaction with simple order: The reaction whose rate only depends on the concentration of reactants, and both the partial order and the reaction order is zero or plus integer is called reaction with simple order. r = kcn n kinds 0 zeroth-order reaction 1 first-order reaction 2 second-order reaction 3 third-order reaction 5.1 the first-order reaction: Reaction: A P at t = 0 c0 at t = t c Differential rate equation: can be rearranged into: dc k1c dt dc k1dt c Which can be integrated directly c0 ln k1t c c c0 exp(k1t ) c c0 exp(k1t ) 1.0 C / mol dm-3 c~t curve of firstorder reaction 0.8 0.6 0.4 0.2 0.0 0 1000 2000 3000 t/s Half-life c0 c 2 c0 ln k1t c 4000 5000 Only when t , can c 0, which suggests that, the first-order reaction can not complete. ln 2 0.6932 t1 k1 k1 2 ln(C/mol dm-3) 0 lnc ~ t curve of the first-order reaction -1 -2 -3 -4 -5 0 1000 2000 3000 4000 5000 t/s ln c ln c0 k1t The slope of the lnc ~ t curve is the k1 Characteristics of the first-order reaction 1) Unit of k is s-1 2) lnc is in linear proportion to t 3) can not complete 4) Half-life does not depend on c0 Example: 1) Decay of isotopes 226 88 Ra 226 86 Rn 42 He 2) Decomposition 1 N 2 O5 N 2 O 4 O 2 2 3) Isomerization Example: The half-life of the first-order decay of radioactive 14C is about 5720 years. The natural abundance of 14C isotope is 1.1 10-13 mol% in living matter. Willard F. Libby Radiochemical analysis of an object 1960 Noble Prize obtained in USA excavation shows that the 1908/12/17 ~1980/09/08 content Application of 14C for age determinations (radiocarbon dating) Calculate the age of the object. is 0.89 an archeological 14C 10-14 isotope mol%. Isotopes used for radiation dating isotope Half-life isotope Half-life 234Th--205Pb 24 day 235U--207Pb 7.13108 yr 210Pb--205Pb 22 yr 40K--40Ar 1.5 109 yr 14C--14N 5692 yr 238U--208Pb 4.5 109 yr 230Th--208Pb 7.52 104 yr 234Th--208Pb 1.39 1010 yr 87Rb--87Sr 5.0 1010 yr 5.2 Second-order reaction 2A P; A + B P A + B P a b cA= ax cB =bx Differential rate equation: dx k 2 (a x)(b x) dt dCA k 2 CA C B dt dx k2 dt (a x)(b x) x 0 x 0 t dx k 2 dt (a x)(b x) 0 x t dx dx k 2 dt 0 (a b)(b x) (a b)( a x) 0 ln( b x) ln b ln( a x) ln a k 2t ( a b) ( a b) ( a b) ( a b) 1 b( a x ) ln k 2t (a b) a(b x) When a = b dc k2 c 2 dt dc 2 k2 dt C0 c C 1 1 k2t c c0 C / mol dm-3 1.0 0.8 0.6 0.4 0.2 0.0 0 1000 2000 3000 t/s 4000 5000 c~t curve of second-order reaction When c 0, t , which suggests that, the pure secondorder reaction can not complete, either. Half-life t1/ 2 1 k2 c0 1/C/ mol dm-3 1/c ~ t curve of second-order reaction 50 40 30 20 10 0 0 1000 2000 3000 4000 5000 t/s For pure second-order reaction 1 dc k2 c 2 2 dt 1 1 2k2t c c0 t1/ 2 1 2k2 c0 Characteristics of second-order reaction 1) Unit of k is mol-1dm3s-1 2) 1/c is in linear proportion to t 3) can not complete 4) Half-life 1 t1 c0 2 Increasing the initial concentration of the reactant will shorten the reaction time. Example: 1) dimerization 2) Decomposition 2 HI = H2 + I2 3) recombination 2CH3 = C2 H6 4) esterification CH 3 COOH+C 2 H 5 OH → CH 3 COOC 2 H 5 +H 2 O 5) hydrolysis C12H22O11 + H2O C12H22O11 + C12H22O11 C12H22O11 + H2O C6H12O6 + C6H12O6 In 1850, experiment done by Wilhelmy suggested the rate equation of the reaction is: r k[C12 H22O11 ] r k[C12 H 22 O11 ][H 2O]v Because the amount of water keeps nearly unchanged during the reaction, [H2O] keeps nearly constant, and the rate equation can be then simplified as r k '[C12 H 22O11 ] Pseudo first-order reaction r k[C12 H 22 O11 ][H 2 O]6 [H 3O ] 5.3 third-order reaction 3A P A + B + C P 2A + B P 3A P 1 1 1 2 2 3k3t 2 c c0 1 dc k3 c 3 3 dt 1 1 2 6k3t 2 c c0 1 t1 2 2 k c 3 0 2 For A + B + C P with same initial concentration Differential rate equation dc k3 c 3 dt Integrated rate equation 1 1 2 2k3t 2 c c0 1 1 1 2 2 k3t 2 c c0 3 t1 2 2 k c 3 0 2 Only five third-order gaseous reactions have been observed. 2NO + X2 N2O + X2O; X = H, D 2NO + O2 2NO2; 2NO + X2 2NOX; X = Br, Cl Are these true third order reactions ? r = k [C6H5CHO]2[CN-] r = k [C2H4O][H+][Br-] Hydrolysis of sucrose r k[C12 H 22O11 ][H 2O][H ] During reaction, both [H2O] and [H+] keep nearly constant and the reaction behaves as a first-order reaction. 5.4 zeroth-order reaction A P Differential rate equation c t c0 0 dc k0 dt c0 c k0t dc k0 dt t1/ 2 c0 2k0 When c = 0, the reaction completes, the reaction time is: c0 t k0 The zero-order reaction can complete. C / mol dm-3 1.0 0.8 0.6 0.4 0.2 0.0 0 1000 2000 3000 4000 5000 t/s c ~ t curve for zero-order reaction Characteristics of zeroth-order reaction 1) Unit of k is mol dm-3s-1 2) c is in linear proportion to t 3) can complete 4) When c increases, reaction time will be prolonged. C0 t k0 Examples: Decomposition over catalysts: 1) 2N2O 2N2 + O2 over Pt wire 2) 2NH3 N2 + 3H2 over W wire Photochemical reaction: r=kI I: intensity of radiation 5.5 for nth-order reaction r kc n 1 1 1 { n 1 } k n t n 1 n 1 (a x) a t1/ 2 2n 1 1 A n 1 n 1 (n 1)kc0 c0 For n 1